CHEMISTRY - MME JOHNSON · 2019-04-02 · Identify the creator of the modern periodic table. 8) Know the difference between stable and reactive. Know which families are more reactive

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CHEMISTRY

Block A: History of the atomic model

1) Describe how historical ideas and models have furthered our understanding of the nature of matter. Describe the contributions from:

a) Ancient Greek Philosophers g) Cavendish b) Alchemists h) Dalton c) Bacon i) Thomson d) Boyle j) Rutherford e) Priestley k) Bohr f) Lavoisier l) Quantum model

Block B: Atoms & Elements

2) Define the word element. Identify the names and symbols of the first 20 elements and Fe, Ni, Cu, Zn, I, Ag, Sn, Au, W, Hg, Pb, U.

3) Identify a proton, electron and neutron from a drawing of an atom. Indicate their: - charge (positive/negative/neutral) - mass (1 amu or negligible) - role in an atom

4) Identify the following characteristics of an element:

- Number of protons - Number of electrons - Number of neutrons - Atomic number (number of protons) - Atomic mass (number of neutrons + protons)

5) Create a Bohr diagram for the first 20 elements.

Block C: The periodic classification of the elements

6) Identify the difference between periods and families. Identify the name of 5 families. Know what a period and a family represent.

7) Identify how elements are arranged in the periodic table. Identify the creator of

the modern periodic table.

8) Know the difference between stable and reactive. Know which families are more reactive than others.

Block D: Compounds

9) Compare the similarities and differences of elements and compounds.

10) Count the number of each atom in a chemical formula. Ex. CO2

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Block E: Properties of substances

11) Identify the properties of metals, nonmetals and metalloids (ductile, conductivity, luster, reactivity). Find them on a periodic table.

12) Study the properties of substances and explain the importance of knowing these

properties.

13) Know what a bond is and the difference between ionic and covalent.

Block F: Chemical changes

14) Distinguish chemical from physical changes.

15) Conduct an experiment to determine the indicators of a chemical reaction. (Change in color, precipitate, heat, gas, light, new substance).

16) What are some natural phenomenon and technologies that use chemical reactions? (Photography, rusting, photosynthesis, combustion).

Block G: Lab Safety

17) Identify the meaning of WHMIS. Where is it used? Know the symbols.

18) Know how to safely work in a lab.

VOCABULARY Atom Stable octet Oxidation Element Mendeleev Corrosion Compound Period WHMIS Molecule Family or Group MSDS Mixture Alkali metals Name/symbol 1st 20 elements + Proton Alkaline earth metals Fe, Ni, Cu, Zn, I, Ag, Sn, Au, W, Electron Chalcogens Hg, Pb, U Neutron Halogens Nucleus Noble gases Isotope Metals Atomic number Metalloids Atomic mass Nonmetals Electron shell Ductile Bohr diagram Luster Valence electron Malleable Ion Reactivity Cation Metallurgy Anion Physical change and properties Bond Chemical change and properties Ionic bond Precipitate Covalent bond Combustion

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HISTORICAL IDEAS ABOUT THE NATURE OF MATTER

Ancient Greek Philosophers

The ancient Greek philosophers wondered why matter behaves as it does and manipulated ideas in their minds but did almost no _______________________.

Empedocles

450 BCE

Proposed that matter was composed of four elements: Earth, Water, Air, _____________.

Democritus

400 BCE

Suggested matter was made of tiny particles that could not be ___________ down any further.

He called them “atomos” which means indivisible. Aristotle

350 BCE

After Democritus died, Aristotle rejected the atomos model and returned to the 4 element model.

This model influenced and dominated scientific thinking for almost _________________ years.

Alchemists

500 – 1600 AD

First people to perform hands-on experiments.

Part philosopher, mystic, _____________________ and chemist.

Three main beliefs: 1. Some elements can be changed into others.

(They were trying to change base metals into _____________). This led them to discover new elements and learn more about existing ones.

2. There was a substance that would give them _________________ life.

3. There was a __________________ solvent that would dissolve all substances.

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Modern Chemists

1600 – present

Use the ______________________ ______________ and experimentation to determine properties of pure substances and explain their composition.

Sir Francis Bacon (1600s)

One of the first scientists to develop new knowledge as a result of experimentation.

Robert Boyle (1650)

Believed the Greek philosophers’ four-element theory could be improved.

Helped lay the foundation for the concepts of elements and compounds.

Recognized that elements can be combined to form ___________________________.

Believed that air was not an element, but a ___________________________ of elements.

Joseph Priestley (late 1700s)

First person to scientifically isolate _______________, but did not know oxygen was an element.

Antoine de Lavoisier (late 1700s)

Defined the term “ELEMENT” as a pure substance that could not be broken down into simpler substances.

Discovered & identified _____________ elements.

Investigations were based on careful measurement and observations.

Recognized that mixtures exist, and identified air as a mixture of oxygen and some other gas.

Henry Cavendish (late 1700s)

Experimented with mixing metal with acid, which produced a flammable gas called ___________________________.

Discovered that hydrogen would burn in oxygen and create water.

Until this time, ________________ was thought to be an element.

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MODELS OF ATOMIC STRUCTURE

John Dalton’s Model of the Atom (early 1800s)

“____________________ Ball” model

All matter is made up of atoms which are too small to see.

Each element has its own kind of atom.

Atoms of different elements are different.

Atoms of different elements can join to form compounds.

Elements were classified according to their ______.

Joseph Thomson (1904)

“Plum __________________________” model

An atom is a sphere of ______________________ charges with negative charges scattered through it.

Ernest Rutherford (1911)

Most of an atom is ____________________ space.

Discovered a tiny, very dense nucleus that contains _____________________ and positive protons.

Surrounding the nucleus is a region of fast moving, negative __________________________.

Niels Bohr (1913)

_____________________________ model

Expanded Rutherford’s model to include electrons have different amounts of ___________________ which allows them to move in different orbits with different energy levels.

________________ are at different distances from the nucleus (like planets and the sun).

Quantum Wave Model

______________________, Planck, Schrodinger, etc.

The structure of matter is of a spherical standing _______________.

Electrons are found 90% of the time in their orbitals.

Smaller particles exist such as quarks and _________________________.

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BLOCK B: ATOMS AND ELEMENTS

Atoms and Their Parts

Everything in existence is __________________.

All matter is made up of ____________________. o Atoms are the smallest particle of any type of matter that still

retains characteristics of that element.

Subatomic Particles:

particles smaller than atoms, no chemical properties of their own ___________________

positively charged particles found in the nucleus of an atom

___________________ particles with no charge, found in the nucleus of an atom

___________________ negatively charged particles moving around the nucleus of an atom

_____________ – the center of an atom where the neutrons and

protons are found (which also gives the atom its mass).

Opposite charges attract so the negative electrons are held in their orbit by the positive protons.

o For Each Element On Your Periodic Table… Protons = the atomic number Electrons = the number of protons Neutrons = atomic mass subtract the number of protons

The largest atom has a diameter of 0.0000005 mm.

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Imagine… o an atom is magnified to the size of the Skydome o the nucleus would be the size of a baseball inside that stadium o the protons would be marbles inside the baseball o the electrons would be mosquitoes buzzing around the baseball o therefore, an atom is mostly empty space

amu stands for ______________________________________ o an amu is a very small unit used to measure the weight of

subatomic particles o 1 amu = 1.66 x10-27kg or 0.00000000000000000000000000166 o an electron is so light, it is not used in the calculation of an

atom’s mass o _______________________ = Protons + Neutrons

Subatomic

Particle Charge Mass Location

Number

determined by… Role in the atom

proton positive

(+) 1 amu Nucleus Atomic number

Identify the element, give

mass, attract electrons

neutron neutral 1 amu Nucleus Mass - protons Give mass, stabilize the

nucleus

electron negative

(-)

1/1837

amu

Electron

shell

Number of protons

(if neutral atom)

Reactivity (making

molecules)

Periodic Table Notation

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ATOM MATCHING AND TRUE/FALSE MATCHING Complete each statement using a term from the list below. Some answers may be used more than once. outside neutrons same cancel out protons atoms negative electrons nucleus lighter no positive

1. All matter is made of tiny parts called _________________________________.

2. The center part of an atom is called the _______________________________.

3. A nucleus is made up of ___________________ and ____________________.

4. Electrons are found ____________________________ the nucleus.

5. Electrons are _____________________________ than protons and neutrons.

6. The main parts of an atom are __________________, ____________________ and _________________________.

7. Since protons have a _________________________ charge, and neutrons have __________________ charge, the nucleus will have a _____________________ charge.

8. Electrons have a _____________________________ charge.

9. An atom has the ___________________________ number of protons and electrons when its overall charge is neutral.

10. The positive and negative charges of an atom _________________ each other.

TRUE OR FALSE? _______ 1. A proton is found outside the nucleus. _______ 2. A proton has a negative charge. _______ 3. A neutron has a positive charge. _______ 4. An electron has a negative charge. _______ 5. An electron is found inside the nucleus. _______ 6. The mass of an atom is the number of protons and neutrons. _______ 7. The atomic number of an atom is the number of neutrons.

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ATOM PRACTICE PROBLEMS

1. Write standard atomic notation for the following (make a box as you would see it in the periodic table).

a. An atom of nitrogen with 7 protons and 8 neutrons

b. An atom of bromine with 35 protons and 36 neutrons

c. An atom of sulfur with 16 protons and 16 neutrons

2. Draw an atom with 6 protons, 7 neutrons and 6 electrons.

3. Which subatomic particles identify an atom/element?

4. Which subatomic particles make up the mass of an atom?

5. If the same charges repel each other, how is it that protons can all be together in the nucleus?

6. Electrons move around with lots of energy. How is it that they do not fly away from their atom?

7. Which subatomic particles will find it easiest to interact with other atoms?

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ATOM CALCULATIONS

Atomic number = # of protons = # of electrons

Atomic mass = # of protons + # of neutrons

# of neutrons = mass – atomic number

Each row in the table represents a different atom. Fill-in the blanks using your periodic table and the above formulas

Number of protons in the atom

Number of electrons

in the atom

Number of neutrons

in the atom

Atomic mass of the atom

Atomic number of the atom

Name of the element

Element symbol

5 11 boron

23 11 Na

79 197 gold

34 45 Se

1 1 1

6 6

92 146

24 12

18 40

110 W

27 aluminum

201 80

7 7

33 42

8 O

Create your own table with only certain boxes filled-in. Exchange your table with a classmate to complete the one they created.

Protons Electrons Neutrons Atomic mass

Atomic number

Element name

Element symbol

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THE ELEMENTS

Element: a pure substance that cannot be chemically broken down into simpler substances.

There are 118 elements, 92 can be found in __________________, 26 are only made in a _______________.

In 1817, Jons Jakob Berzelius proposed an international system of symbols.

Symbols are much _________________ and faster to use than writing out the names of each element. Ex. Hydrogen and oxygen make hydrogen peroxide. H2 + O2 → H2O2.

Element symbols are the same across ______________________ but names are specific to each language. Ex. Silver (English) = Ag (symbol) = Argent (French). Languages that use different written characters (like Chinese), still use these symbols.

An element is __________________ by the person that discovers it. Names come from the following:

1. A Greek word: Ex. Chlorine from chloros which means _______. Argon from argos which means inactive. Helium from helios which means __________.

2. A Latin word: Ex. Sodium Na _____________

Potassium K kalium Antimony Sb stibium Copper Cu _____________ Gold Au aurum Silver Ag argentums ____________ Fe ferum Lead Pb plumbum Mercury _____ hydrargyrum Tin Sn stannum

3. A country: Ex. Polonium Po Poland

___________ Ge Germany Francium Fr France

4. A continent: Ex. Americium Am Americas

Europium Eu Europe

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5. A person Ex. Einsteinium Es Albert Einstein

Rutherfordium Rf E. Rutherford ____________ Cm Marie Curie Fermium Fm Enrico Fermi

Symbols are assigned by the following rules: 1. The first letter of the element name. Ex. C = carbon.

2. The first and second letter of the element name if the first is already taken. Ex. Ce = cerium.

3. The first and third letter of the element name if the first two are already taken. Ex. Cs = cesium.

4. Some symbols follow the above rules but with their latin or greek root. Ex. Tungsten = W = Wolfram (the German name)

5. Some symbols do not follow the rules and just need to be memorized. Ex. Platinum should be Pl but it is Pt. Ex. Zirconium should be Zi but it is Zr.

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ELEMENT BINGO Randomly place 25 of the symbols below in the BINGO grid.

S F B Pb Cl H Cr Au Be P Na Ar He O Li Ca Hg W I N Mg C Cu Zn Co Fe Mn Sn Ag Br Ne Al Si K

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ELEMENT SCRABBLE

Name: ______________________________ _____/30

Goal: to become more familiar with the periodic table and the elements.

Instructions: Create words using the symbols in the periodic table. You must write the word as the symbols are written in the table (capitals and lower case). You may not have the same answers as other students. Example: BaNaNa – barium, sodium, sodium Create 3 words with 4 letters: Word Names of elements

1. _________________ - ______________________________________________

2. _________________ - ______________________________________________

3. _________________- ______________________________________________ Create 3 words with 5 letters: Word Names of elements

1. _________________ - ______________________________________________

2. _________________ - ______________________________________________

3. _________________ - ______________________________________________ Create 3 words with 6 letters: Word Names of elements

1. _________________ - ______________________________________________

2. _________________ - ______________________________________________

3. _________________ - ______________________________________________ Create 3 words with 4 or more letters: Word Names of elements

1. _________________ - ______________________________________________

2. _________________ - ______________________________________________

3. _________________ - ______________________________________________ Create 3 new words and include a definition: Word Names of elements and the definition of the word

1. _________________ - ______________________________________________

2. _________________ - ______________________________________________

3. _________________ - ______________________________________________

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BOHR MODELS

Order of electron placement.

STEPS TO DRAW A BOHR DIAGRAM

Example: Nitrogen

1) Find the number of electrons for that element. How? If the atom is neutral, the number of electrons is the same as the number of protons which is also the atomic number.

- Nitrogen’s atomic number = 7 = number of electrons

2) Write the symbol for the element and the number of protons and neutrons.

- N7protons 7neutrons Neutrons = mass – protons = 14 – 7 = 7 neutrons

3) Begin to fill the level closest to the nucleus with electrons. Make sure a level is full before beginning the next level.

4) There are 7 electrons in nitrogen. The first level will have 2 electrons as far apart as possible because the charges repel each other. The second level has 5 electrons. 4 are placed opposite each other and the fifth is placed in a pair.

N7p7n

Examples: 1) Aluminum (Al) 2) Sodium (Na)

1

5

3

6

7

13

11 15

14

12 16

2

4 8

9 10

17 18

A Bohr diagram is used to give a general idea of where electrons are found in an atom.

Electrons are drawn in energy levels (orbits). The closest level to the nucleus has the lowest amount of energy.

Electrons circle the nucleus in a random fashion to create a cloud. They do not circle in a predictable fashion like the planets and the sun.

Electrons = dots Energy level = circle

1st level can hold up to 2 electrons

2nd level can hold up to 8 electrons

3rd level can hold up to 8 electrons

4th level can hold up to 18 electrons

When a level has more than 4 electrons, the electrons are drawn in pairs.

Each level must be full before filling the next level.

Indicate the number of protons and neutrons in the nucleus.

NAME:___________

BOHR MODEL PERIODIC TABLE1

Hydrogen

3

Lithium

4

Beryllium

5

Boron

6

Carbon

7

Nitrogen

8

Oxygen

9

Fluorine

10

Neon

11

Sodium

12

Magnesium

13

Aluminium

14

Silicon

15

Phosphorus

16

Sulfur

17

Chlorine

18

Argon

19

Potassium

20

Calcium

1) What do all of the columns have in common?

2) What do all of the rows have in common?

2

Helium

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BLOCK C: THE PERIODIC TABLE

History of the Periodic Table

The first periodic table was made by Dimitri Mendeleev in 1869. He ordered the

elements according to their _____. Some spaces were left empty because he predicted

that there were other elements yet to be discovered. In the current periodic table, the

elements are in ascending order according to their ___________ number (# of protons).

Metals, non-metals and metalloids

Most elements are metals. They are found on the ____________ of the table. The right

side of the table contains the __________________. Metalloids share characteristics of

metals and non-metals and are found between the two on what is called the “staircase”.

1 H

2 He

3 4 5 6 7 8 9 10

Li Be B C N O F Ne

11 12 13 14 15 16 17 18

Na Mg Al Si P S CI Ar

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe

55 56 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg TI Pb Bi Po At Rn

Metals (to the left of the staircase)

- _______________________

- Good __________________________ of heat and electricity

- _______________________ (can hammer or press out of shape and not shatter)

- _______________________ (can be stretched into a wire and not lose strength)

- ___________________ of electrons to other elements

- React with _____________________

- All are _________________ at room temperature except mercury (liquid)

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Non-metals (to the right of the staircase)

- _______________ (not shiny)

- Not good conductors of heat and electricity

- Like to _____________________ electrons from other elements

- All are __________________ at room temperature except carbon, iodine, sulfur,

selenium and phosphorus (solids) and bromine (liquid)

Metalloids (staircase)

- Characteristics fall somewhere between those of metals and non-metals

- All are ____________________ at room temperature

- There is debate over whether ___________________ is a metalloid or non-metal

because it is so unstable. It doesn’t last long enough to study it.

- Considered ___________________________

Hydrogen is an ______________________ and is considered a non-metal most of the

time. Sometimes it has qualities like a metal and other times it is more of a non-metal (it

is a gas at room temperature). It can give or receive an electron.

1 2

H He

3 4 5 6 7 8 9 10

Li Be B C N O F Ne

11 12 13 14 15 16 17 18


19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36


37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54


55 56 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86


87 88 103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118

Fr Ra Lr Rf Dd Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og

57 58 59 60 61 62 63 64 65 66 67 68 69 70

La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb 89

90 91 92 93 94 95 96 97 98 99 100 101 102

Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No

Metals

Metalloids

Non-metals

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Families in the Periodic Table

- each ______________________ in the table is a family of elements

- another word for family is group

- each element in a family has the same number of valence electrons

- valence electrons are the electrons found in the __________________ energy

shell that can move from one element to another to form a chemical bond

- the Roman numeral above a family indicates the number of valence electrons

- elements in a family have similar ______________________________

Alkali metals (group 1)

- soft, highly ______________________ metals

- like to bond with the __________________ family and give away _____ electron

- ____________________ is an exception because it can behave like a non-metal

Alkaline earth metals (group 2)

- malleable, reactive, burn easily

- like to bond with the _____________________ family and give away 2 electrons

Chalcogens (group 16)

- like to bond with the alkaline earth metals and receive ____________ electrons

Halogens (group 17)

- highly reactive, especially with the alkali metals where they gain an electron

- like to form _______________ compounds

Noble gases (group 18)

- very ________________________ gases

- do not like to react with other elements because their electron valence layer is

_____________

- found in their natural state

Periods in the Periodic Table

- each period is a ___________________________ row in the table

- the number of each row is equal to the number of energy levels for each element

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Question

Use the table below to colour the different families. Make sure to include a legend.

Leave the newer elements at the bottom (#116 - #118) blank as scientists are not sure if

they demonstrate the characteristics of those families.

1 2

H He

3 4 5 6 7 8 9 10

Li Be B C N O F Ne

11 12 13 14 15 16 17 18


19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36


37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54


55 56 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86


87 88 103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118

Fr Ra Lr Rf Dd Sg Bh Hs Mt Ds Rt Cn Nh Fl Mc Lv Ts Og

57 58 59 60 61 62 63 64 65 66 67 68 69 70

La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb

89 90 91 92 93 94 95 96 97 98 99 100 101 102

Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No

Legend

Alkali metals

Alkaline earth metals

Chalcogens

Halogens

Noble gases

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ATOMS AND ELEMENTS PROBLEMS

1. Draw the Bohr diagrams of the energy levels for the following elements.

2. Draw the Bohr diagrams of the energy levels for the alkali metals.

3. What is similar between all the alkali metals in question #2? ______________________________________________________________

______________________________________________________________

4. From one period to the next, what happens to the number of energy levels?

______________________________________________________________

______________________________________________________________

5. How many valence electrons does Rubidium (Rb) have? ________________

6. How many energy levels does Rubidium (Rb) have? ___________________

7. Draw the Bohr diagrams for the first 3 elements of each of these families.

Alkali metals Alkaline earth metals Noble gases

Li

O

Na

Ar

Ca

3 18 20 11 8

H

Li

Na

K

19 3 1 11

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8. What similarities can you find between all the elements of the same family?

______________________________________________________________

______________________________________________________________

9. What differences can you find between all the elements of the same family?

______________________________________________________________

______________________________________________________________

10. What is the difference between a neutral atom and a stable atom?

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________

11. What is a valence electron?

______________________________________________________________

______________________________________________________________

12. Which family of elements do you think is the most stable? Why?

______________________________________________________________

______________________________________________________________

13. a) Who created the first periodic table? ______________________________

b) What was different about his table and the current periodic table?

___________________________________________________________

___________________________________________________________

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ELEMENT CARDS PROJECT

In this project, you will research 4 different elements using the Internet and your

periodic table. (15 points per element x 4 elements = 60 points)

Each element card must include: _____ 1. Information from the periodic table (ex. Atomic number, atomic

mass, name, symbol, state – solid/liquid/gas). 2 points _____ 2. The number of protons, neutrons and electrons. 3 points _____ 3. The name of the family it belongs to. (If it doesn’t have an official

name, the family is named after the first element in that column, for example, the carbon family). 1 point

_____ 4. Is it a metal, metalloid or non-metal? 1 point _____ 5. The people who discovered it and the date. 2 points _____ 6. At least 3 important uses for the element. 3 points _____ 7. At least 1 image showing how the element is used. 1 point _____ 8. Neatly written and displayed. Easy to follow. 2 points

P = _____ N = _____ E = _____

Family name: __________________

Metal ___ Metalloid ___ Non-metal ___

Discovered in _______ by

_________________________

Uses:

Images on the back

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O Oxygen 15.9994

Gas

Determine the number of protons,

neutrons and electrons.

Indicate the date the element was

discovered and the person or group

who discovered it.

Give at least 3 uses of the element.

Show one or more images on the back

demonstrating how the element is

used.

Fill in this square with the information

from the periodic table.

Give the family name.

Indicate if the element is a metal,

metalloid or non-metal.

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BLOCK D: ELEMENT OR COMPOUND?

Matter

1 type of atom 2 or more types of atoms bonded together bonded together

Element Compound

Ex. _____________

Ex. _____________

Monoatomic Diatomic Polyatomic

1 atom 2 of the same 3 or more of the atom same atom Ex. ______ Ex. ____________ Ex. _________ ____________ ____________

Similarities

(elements & compounds) Differences

(elements & compounds)

1. Both are made of matter so they both have a mass and are made of atoms.

2. Both are pure substances and each have their own properties.

3. Both can be found naturally in pure forms but more often are in mixtures.

4. Pure elements and compounds can be made artificially.

5. Both can be represented by symbols and chemical formulas.

1. Elements are one type of atom. Compounds are 2 or more different types of atoms.

2. Elements can contain one, two or many atoms of the same type, while a compound always has different types of atoms.

3. The properties of a compound are different than the individual properties of each of its elements.

4. A compound’s properties are determined by its composition and structure (ex. CO2 and CO are different)

5. There are only 118 elements but 10 million or more pure compounds.

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COUNTING ATOMS How do chemists represent the number of atoms in a molecule? Or the number of molecules? Or the structure of those molecules? Chemists will use the following: Subscript:

- __________ bottom number - Represents the number of atoms of the element directly to the

___________. - No subscript represents the number 1, it is implied by the symbol. - All atoms written together with and without subscripts, are all joined

together to make up a molecule. - Ex. H2O ___ H ___ O There is one molecule of water.

Coefficient:

- _____________ number before the molecule - Represents how many molecules you have (of the molecule that is

written right after it). They are not attached together. - Multiply the _________________ for each atom by the coefficient - The number 1 is not written, it is implied. - Ex. 2CO2 _____C _____ O There are 2 separate carbon

dioxide molecules.

Parentheses:

- Represents more than one _______________ in a molecule. - Multiply each atom in the parentheses by the ______________ on

the outside. - Ex. Mg(NO2)2 ____ Mg ____ N ____O

One way of saying this is “there are 2 groups of NO2 in a magnesium nitrite molecule”. All these atoms would be joined together to make one molecule.

H H

O

O O

C

O O

C

O O

N Mg

O

N

O

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Explain the difference between the molecules below by counting the atoms in each one.

a) CO2 ____ C _____ O

b) CoCO

____ Co _____ C _____ O

c) Co2 ____ Co

d) 2CO

____ C _____ O

e) Fe2(CO3)3

____ Fe _____ C ______ O

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CHEMICAL FORMULAS PRACTICE For each of the elements in the left column, answer the questions in the two other columns. You may use a molecule building set if you would like to construct each one.

Chemical Formula

a) How many different kinds of atoms are in this molecule? b) How many atoms of each kind are in this molecule? c) What is the total number of all atoms in this molecule?

What does this molecule

represent?

Water H2O

a) b) c)

□ a pure substance □ a compound □ a monatomic element □ a diatomic element □ a polyatomic element

Carbon dioxide CO2

a) b) c)


Calcium carbonate CaCO3

a) b) c)


Sodium chloride NaCl

a) b) c)


Oxygen O2

a) b) c)


Ozone O3

a) b) c)


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Hydrogen peroxide H2O2

a) b) c)


Manganese sulfate MnSO4

a) b) c)


Nitrogen N2

a) b) c)


Vinegar (acetic acid) CH3COOH

a) b) c)


Sulfur S8

a) b) c)


Neon Ne

a) b) c)


Methane CH4

a) b) c)


Calcium iodide CaI2

a) b) c)


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Diamond C

a) b) c)


Rust (iron hydroxide) Fe(OH)2

a) b) c)


Glucose C6H12O6

a) b) c)


Ammonia NH3

a) b) c)


MORE QUESTIONS

1. How many atoms in 6 AlCl3?

2. How many molecules in 3 MgBr2?

3. How many atoms in 2 PCl2?

4. How many molecules in 4 AlCl3?

5. How many chlorine atoms in 5 PCl2?

6. How many magnesium atoms in 3 MgBr2?

7. What is the ratio between the atoms in AlCl3?

8. What is the ratio between the atoms in 6 AlCl3?

9. What is the ratio between the atoms in 2 P2Cl5?

10. True or false? A molecule is only made up of two elements.

11. True or false? A molecule can contain many atoms of the same element.

12. True or false? In 6 H2O, there are 6 molecules of water.

13. True or false? In 3 NH3, there are 3 atoms of hydrogen.

14. True or false? CO is an element.

15. True or false? Co is a compound.

30

BLOCK E: PROPERTIES OF SUBSTANCES

Matter: anything that occupies a _______________________ and has a ___________.

Example: air and a rubber soccer ball.

Properties of matter

The properties of matter can be separated into 2 categories: physical properties and

chemical properties.

Qualitative physical properties

Physical properties of matter are observed with our five _________________ (vision,

hearing, taste, smell and touch). Physical properties of matter can help to

_____________________ a substance. Example: colour is a physical property.

States of matter: matter is found in one of the following states at room

temperature – solid, liquid or gas.

Solid: has a defined form and a stable __________________________.

Liquid: always conforms to the shape of its ________________________

and has a stable volume.

Gas: always adopts the shape of its container and __________ it completely.

Durability: Durability indicates a solid’s inability to __________________ or dent.

A more durable material can be used to scratch a less durable material. Example:

using a diamond to scratch glass.

Malleability: If a solid is malleable, it can be ___________________________

into thin sheets. Gold can be hammered into thin sheets so it is said to be

malleable. Glass is not malleable. If it is hammered, it breaks into pieces.

Ductility: The ability of a material to be pulled into thin __________________. For

example, copper is ductile because it can be pulled into wires for electrical wiring.

Crystals: some solids can be organized in regular _______________________.

When looking at a crystal, you can see distinct geometric patterns, such as cubes.

For example, under a microscope, table salt looks cube shaped.

Quantitative physical properties

These are properties that must be measured.

Boiling point and melting point: the temperature at which a substance changes

from one _________ to another. The melting point is the temperature when a solid

changes to a liquid (or vice versa). The boiling point is when a liquid changes to a

gas (or vice versa). Water has a melting point of 0 ºC and a boiling point of 100 ºC.

31

Solubility: The ability for a substance (solute) to ________________ in a solvent.

If you add salt and pepper to water, the salt dissolves in the water and not the

pepper.

Viscosity: the __________________ of a liquid or its inability to run down an

incline. The thicker the liquid, the more viscous it is. For example, syrup is more

viscous than water.

Density: Density is the quantity of __________________________ per unit of

____________________. For example, lead has a larger density than a feather. It

is measured in g/cm3.

Chemical properties

A chemical property describes the behaviour of a substance when it comes into contact

with another ____________________ or energy source. The change that occurs is not

reversible. For example, dynamite that explodes.

Combustible (or flammable): a substance is combustible if it can be

______________________ when exposed to a flame.

Reacts with acids: the ability to react with an acid is a chemical property. The

majority of ______________________ react with acids.

Corrosion: when a metal reacts with an ______________________ substance.

For example, iron reacts with oxygen to become rust.

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QUESTIONS: Physical and Chemical Properties

1. What is the difference between qualitative physical properties and quantitative

physical properties?

2. Give 3 qualitative physical properties of an orange.

3. Give 3 quantitative physical properties of water.

4. Indicate which of the statements below are quantitative and which ones are

qualitative.

a. The density of air is 1.5 g/L. ___________________

b. The boiling point of nitrogen is -196°C. ______________________

c. Table salt is a white solid. _____________________

5. Indicate which of the following statements are examples of physical

characteristics and which ones are chemical characteristics.

a. Calcium is a metal that is fairly soft. ______________________

b. Calcium reacts with water. _______________________

c. Snow is a solid. _______________________

d. Ozone is toxic for humans. _____________________

e. Sodium bicarbonate reacts with acids. _______________________

f. Mercury is toxic. _______________________

g. Paper burns easily. _________________________

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CHEMICAL BONDS

A ________________ is a force that attracts atoms to one another in a chemical

compound (or molecule).

A bond forms between two atoms due to the interaction of the atoms’ valence electrons.

A bond forms a compound that is more stable than the atoms by themselves. Many of

the elements in the periodic table do not exist in nature as single atoms, rather they are

a part of compounds.

**Metals tend to lose electrons. They form positive ____________ (an atom with a

charge) called ________________________.

**Non-metals tend to receive electrons. They form negative ions called _____________.

1. Ionic bonds

This type of bond forms when electrons are __________________________ between

two atoms. One atom loses one or more electrons and the other atom receives them.

This bond occurs between a __________________ and a ______________________.

Ex : NaCl and MgO

Example: Salt is sodium chloride or NaCl.

Na (sodium) and Cl (chlorine) atoms:

Sodium 1123 Na Chlorine 17

35Cl

- electrons: ______ - electrons: ______

- protons: ______ - protons: ______

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In sodium chloride:

Sodium Chlorine

- electrons: ______ - electrons: ______

- protons: ______ - protons: ______

electric charge: _______ electric charge: ______

An anion is an atom or group of atoms ______________________________________ _____________________________________________________________________. A cation is an atom or group of atoms _______________________________________ _____________________________________________________________________. 2. Covalent Bond

This type of bond __________________ electrons between atoms. It occurs between

two ______________________________ (or metalloids).

Ex: HCl, I2 and O2.

This is a positive ion:

a cation Na +

This is a negative ion:

an anion Cl —

A compound is composed of atoms joined together by ionic bonds. Another name for this is an ionic compound. A compound made-up of covalent bonds is called a

molecule.

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QUESTIONS: Ionic Bonds 1. Using the word bank below, complete the sentences in the paragraph below.

Attraction, charge, electron, ionic bond, positive, positive charge, negative, negative charge, transferred, opposing.

When an atom receives or loses an ___________________, an ion is formed. All ions

have a ____________. Metals have a tendency to form ions with a ________________

________________________ while non-metals have a tendency to form ions with a

__________________________________. When a metal atom reacts with a non-metal

atom, one or more electrons are ________________________, this causes ions to

form. There will be ___________________ ions and ___________________________

ions. The ions are attracted to each other due to their __________________ charges.

This is what we call an _________________________.

2. a) Draw a Bohr diagram for lithium in the space below.

b) What will cause lithium to become an ion? __________________________________

______________________________________________________________________

c) The ion that forms, will it be positive or negative? Explain why. _________________

______________________________________________________________________

3. a) Draw a Bohr diagram for fluorine in the space below.

b) What could happen that would change fluorine into an ion? ____________________

______________________________________________________________________

c) The ion that forms will be positive or negative? Explain. _______________________

______________________________________________________________________

4. Lithium and fluorine react together to form lithium fluoride. With the help of a Bohr

diagram, draw how these two atoms react.

36

5. The following diagram represents an oxygen atom. It can be used to answer the

following questions.

a) Why is this atom unstable? _________________________________________

b) What will make this atom stable? _____________________________________

c) With a red pen, modify the diagram so it shows a stable atom.

d) What is the charge of this atom? _____________________________________

QUESTIONS: Covalent Bonds

1. What does the small circle (A) represent? _____________________________

2. What does the large circle (B) represent? _____________________________

3. What does C represent? __________________________________________

4. How many electrons are in the valence layer for the atom on the left? ______

5. How many electrons are in the valence layer for the atom on the right? _____

6. What is the difference between an ionic bond and a covalent bond? __________

________________________________________________________________

7. Draw Bohr diagrams to show how the following atoms join together with covalent

bonds.

H2

FCl

A

B

C

37

OF2

NH3

8. Why do the noble gases, like He and Ne, not bond with other atoms?

________________________________________________________________

9. Identify if the following molecules are held together by ionic bonds or covalent

bonds. i. NaBr ______________________ ii. N2 ______________________ iii. LiF ______________________ iv. CO2 ______________________ v. CCl4 ______________________ vi. BeO ______________________

10. Identify if the following ions are cations or anions. a) Na+ __________________________ b) Cl- __________________________ c) S2- __________________________ d) F- __________________________ e) Fe2+ __________________________ f) Ni3+ __________________________ g) O2- __________________________

38

BLOCK F: PHYSICAL AND CHEMICAL CHANGES

Physical changes:

- do not make a new ______________________

- the substance may change appearance but its ________________ is the

same. Ex. Tearing a piece of paper. Dissolving a substance in water.

- a change of _________________ (gas, liquid, solid) is a physical change

Ex. Ice melting

Chemical changes:

- atoms are rearranged to create new ________________________ with new

_________________________

Indicators of a chemical reaction

Releases a _________________ (bubbles)

Changes ___________________

Makes a _____________________ (a solid that forms in the bottom of a liquid)

Releases __________________ (heat or light)

Creates an ___________________

Very difficult to __________________

Often, more than one indicator of a chemical reaction needs to be seen to confirm it is a chemical change and not physical. For example, releasing a gas could be a physical change (such as when boiling water). Just a few examples of chemical reactions:

Baking a cake

A rusting nail

Burning wood

Glow sticks are an example of ____________________________

___________________________

6H2O + 6CO2 + energy → C6H12O6 + 6O2

Notice in this chemical reaction there is the same amount of type of atom on both

sides of the arrow. This is because atoms cannot be created or destroyed during

a chemical reaction – only rearranged.

Brainstorm some more chemical reactions.

Chemical reactions in nature Chemical reactions in technology

39

Questions: Chemical and Physical Changes

Classify each of the following changes as physical or chemical. Justify your answer.

SITUATION TYPE OF CHANGE JUSTIFICATION

1. Gina hangs her bathing suit and towel on the clothes line. Two hours later they are dry.

This is a: __ physical change __ chemical change

2. Marvin returns home from a vacation to find the margarine left in the fridge has a strange smell.


3. Nathalie is very sad that her chocolate bar melted on the dashboard of her car.


4. Keith mixes a white powder with a colourless acid. A purple precipitate appears in the bottom of the beaker.


5. Andrea uses caulking to fill a crack between the window and the wall. It hardens in less than an hour.


6. Rauno mixes a red powder with a colourless acid. The next day there is still a red powder in the bottom of the beaker and the colourless acid around it.


40

7. Beatrice is building a bookshelf and is covered in sawdust at the end of the day.


8. Somchine prepares a traditional Laotian meal for his friends. He is proud of his spicy chicken.


9. Yasmin brings a salad to Somchine’s dinner. The salad has 7 different vegetables cut into tiny pieces.


10.Thierry likes to surprise his friends by lighting firecrackers with a rock.


11. When George’s father makes wine from crab apples, bubbles form on the surface of the yeast

and fruit mixture.


12. During a school volleyball game, Jennifer sprains her ankle. Her coach squeezes a bag at room temperature that quickly becomes very cold.

This is a: __ physical change ► chemical change

41

BLOCK G: LAB SAFETY WHMIS

WHMIS (Workplace Hazardous Materials Information System) is a comprehensive system for providing health and safety information on hazardous products intended for use, handling, or storage in Canadian workplaces.

The three focuses of WHMIS are: • Labels on containers for dangerous materials. • SDS safety data sheets for dangerous materials. • Education and training employers and employees. WHMIS PICTOGRAMS

The exclusions under WHMIS 2015 are:

Explosives as defined in the Explosives Act.

Cosmetic, device, drug or food as defined in the Food and Drugs Act.

Pest control products as defined in the Pest Control Products Act.

Consumer products as defined in the Canada Consumer Product Safety Act.

Wood or products made of wood.

Nuclear substances within the meaning of the Nuclear Safety and Control Act, that are radioactive.

Hazardous waste being a hazardous product that is sold for recycling or recovery, or is intended for disposal.

Tobacco and tobacco products as defined in the Tobacco Act.

Manufactured articles. Many of these products are covered under other legislation. Note that while a product may be exempt from the requirement to have a WHMIS label and SDS, employers must still provide education and training on health effects, safe use, and storage.

42

QUESTIONS: WHMIS

What is the risk associated with each symbol?

43

44

CHEMISTRY UNIT REVIEW Block A Name: ___________ ____/80 ***Know the definitions of the vocabulary on the second page of this book***

1. Match the following people with their discoveries. (12 points) _____ Ancient Greeks a) Plum pudding model – mixed electrons and protons _____ Alchemists b) First to isolate oxygen _____ F. Bacon c) Part magicians / chemists. Wanted to make gold. _____ R. Boyle d) Billiard ball model. Elements are different atoms. _____ J. Priestley e) One of first to successfully use experimentation. _____ A. Lavoisier f) Matter made of 4 elements. Particles called atomos. _____ H. Cavendish g) Defined the word element. Identified 23 elements. _____ J. Dalton h) Planetary model. Electrons move in energy levels. _____ J. Thomson i) Made hydrogen and water. Water not an element. _____ E. Rutherford j) Foundation for element / compound definitions. _____ N. Bohr k) Quarks, photons and electron clouds. _____ Quantum Wave Model l) Discovered neutrons.

Block B

2. Where are these found in an atom? (3 points) a) Proton: ____________ b) Neutron: ___________ c) Electron: ____________

3. What charge are these particles? (3 points)

a) Proton: ____________ b) Neutron: ___________ c) Electron: ____________

4. How many amu’s for each of these particles? (3 points) a) Proton: ____________ b) Neutron: ___________ c) Electron: ____________

5. Give one function of each particle. (3 points)

a) Proton: _______________________________________________________ b) Neutron: ______________________________________________________ c) Electron: ______________________________________________________

6. Complete the following table. All elements are neutral. (7 points)

Number of protons in the atom

Number of electrons

in the atom

Number of neutrons

in the atom

Atomic mass of the atom

Atomic number of the atom

Name of the element

Element symbol

12 12

27 59

28 14 Silicon

7. Know the names and symbols for these elements. (0 points)

H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Fe Ni Cu Zn I Ag Sn Au W Hg Pb U

45

8. Draw a Bohr diagram for sodium. (2 points)

9. Draw a Bohr diagram for neon. (2 points)

Block C

10. Who created the first periodic table? ______________________________ (1)

11. The first periodic table was ordered according to ____________ but now it is ordered according to ______________________________. (2 points)

12. Complete the following table from block C in your notes. P.203 Science Power. (10 pts)

METALS METALLOIDS NON-METALS

Position in periodic

table (staircase, left,

right)

State (solid, liquid,

gas)

Ductility (low, high)

Lustre

(dull, shiny,

somewhat shiny)

Malleability

(high, low)

Conductivity

(high, low, semi)

Reactivity

(high, low, semi)

13. Give the names of each family and the number of valence electrons. (5 points)

a) Family 1 - __________________________________. Val. Elec. - _________ b) Family 2 - __________________________________. Val. Elec. - _________ c) Family 16 - _________________________________. Val. Elec. - _________ d) Family 17 - _________________________________. Val. Elec. - _________ e) Family 18 - _________________________________. Val. Elec. - _________

Block D

14. Give two similarities between an element and a compound. (2 points)

46

15. Give two differences between an element and a compound. (2 points)

16. How many of each type of atom are in these molecules? (3 points) a) C6H12O6 ____C _____H _____O b) Fe2(SO4)3 ____Fe _____S _____O c) 3Mg(OH)2 ____Mg _____O _____H

Block E

17. a) An ionic bond is when 2 electrons share / give-take (circle one). (1 pt)

b) A covalent bond is when 2 electrons share / give-take (circle one). (1 pt)

c) An ionic bond is between a metal and non-metal / 2 non-metals (circle one). 1

d) A covalent bond is between a metal and non-metal / 2 non-metals (circle one).

e) Give the definition of an ion: ____________________________________ (1)

f) Give the definition of an anion: ___________________________________ (1)

g) Give the definition of a cation: ___________________________________ (1)

Block F

18. What is the difference between a physical and chemical change? (2 points)

19. Give 5 indicators of a chemical change. (5 points) - - - - -

Block G

20. What do the letters in the word WHMIS stand for? (1 point) W – H – M – I – S –

21. What are 5 safe behaviours or procedures in the lab? (5 points) 1. ______________________________________________________________

2. ______________________________________________________________

3. ______________________________________________________________

4. ______________________________________________________________

5. ______________________________________________________________

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CHEMISTRY - MME JOHNSON · 2019-04-02 · Identify the creator of the modern periodic table. 8) Know the difference between stable and reactive. Know which families are more reactive