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I II IIISMB, Periodic Table Notes 2011 1
The Periodic Table- Topic 5
Click for song
Bellwork: Using your RB (pgs 78-83), define the following words in your notebook: family, group, periodic law, period, metal, metalloid, nonmetal
Mendeleev’s Periodic Table (1869) How did Mendeleev organize his periodic table? The Abbreviated History of the Periodic Table for Reg
ents Chemistry
6.1
SMB, Periodic Table Notes 2011 3
A. Dmitri Mendeleev (1869, Russian) Organized elements by
increasing ATOMIC MASS.
Elements with similar chemical properties were grouped together.
There were some discrepancies.
I. HISTORY
SMB, Periodic Table Notes 2011 4
B. Henry Moseley
ORGANIZED ELEMENTS BY INCREASING ATOMIC NUMBER.
Resolved discrepancies in Mendeleev’s arrangement.
The Periodic Law In the modern periodic table, elements are
arranged in order of increasing atomic number.
6.1
Mendeleev’s original table was according to mass. This was changed when Moseley discovered atomic number.
When elements are arranged in order of INCREASING ATOMIC #, elements with similar chemical properties appear at regular intervals.
The properties of the elements within a period change as you move across a period from left to right.
The pattern of properties within a period repeats as you move from one period to the next.
0
50
100
150
200
250
0 5 10 15 20Atomic Number
Ato
mic
Ra
diu
s (
pm
)
SMB, Periodic Table Notes 2011 7
1. Horizontal rowsCalled PERIODSAll elements in the same period have the same number of ENERGY LEVELS in their atomic structure
A. Arrangement of Table
II. ORGANIZATION OF THE ELEMENTS
SMB, Periodic Table Notes 2011 8
2. Vertical Columns
a) Called GROUPS OR FAMILIESb) All elements in the same group have the
same number of VALENCE ELECTRONS, therefore lose or gain the SAME number of electrons, form similar CHEMICAL FORMULAS and have similar CHEMICAL PROPERTIES
ex. XCl2 Group 2:
Be +2 Cl -1 = BeCl 2
Mg +2 Cl -1 = MgCl2
Remember: When
writing formulas,
use the criss-cross
rule to cancel out
oxidation states
SMB, Periodic Table Notes 2011 9
Elements can be classified by their properties and located on the Periodic Table as metals, nonmetals, metalloids or semimetals
Metals on the left
Nonmetals on the rightMetalloids or semimetals
III. Comparing Metals, Nonmetals & Metalloids
SMB, Periodic Table Notes 2011 10
Elements on the Periodic Table are divided into three subgroups called METALS, NONMETALS and METALLOIDS
(semimetals).
Decrease metallic propertiesDecrease metallic properties
Increase Increase
metallic metallic
propertiesproperties
Increase Increase
nonmetallic nonmetallic
propertiesproperties
Click on
SMB, Periodic Table Notes 2011 11
METALS: located on the LEFT SIDE of the periodic table (except H); MORE THAN 2/3 of all elements
1. Chemical properties tend to LOSE ELECTRONS EASILY have LOW IONIZATION ENERGY (energy
needed to remove electrons) Metallic character INCREASES as
ionization energy decreases. have LOW ELECTRON AFFINITY
(attraction for electrons) form POSITIVE IONS when combining
with other atoms FRANCIUM most reactive metal: See
Table J http://castlelearning.com/review/reference/chem%20table%20j.htm
SMB, Periodic Table Notes 2011 12
2. Metals Physical Properties
good conductors of heat and electricity
LUSTROUS - reflect light, shine when they are polished
MALLEABLE - can be rolled or hammered into sheets
DUCTILE - can be drawn into wires
are SOLIDS at room temperature except for MERCURY (liquid)
SMB, Periodic Table Notes 2011 13
B. NONMETALS
1. Chemical properties tend to GAIN electrons to form
NEGATIVE IONS have high electron affinities
(electronegativity) produce COVALENT bonds by
SHARING electrons with other nonmetals
FLUORINE most reactive nonmetal: see Table J
located on the right side of
the periodic table (except for
Noble gases)
SMB, Periodic Table Notes 2011 14
2. Nonmetals Physical Properties
exist as gases, molecular solids, or network solids at room temperature except BROMINE (liquid)
BRITTLE - (shatters when struck) DULL - does not reflect light even when
polished POOR CONDUCTORS of heat and
electricity Allotropes: Different SHAPE & PROPERTIES
forms from the same element.CARBON: coal; diamond, graphite OXYGEN: O2; O3 (OZONE)
C. METALLOIDS (semi-metals)
Found lying on the jagged line between metals and nonmetals flatly touching the line (except Al and Po).
B,Si,Ge,As, Sb, & Te Exhibit properties of both
metals and nonmetals Behave as nonmetals but
their conductivity is like metals
SEMICONDUCTORS – Si and Ge
SMB, Periodic Table Notes 2011 16
Many properties of the elements change
in a predictable way as you move
through the periodic table – these
systematic trends are called periodic
trends..(use reference Table S for data comparison)
Periodic Trends
SMB, Periodic Table Notes 2011 17
Reference Table S
SMB, Periodic Table Notes 2011 18
© 1998 LOGAL
1. Atomic Radius
DESCRIPTION: ½ THE
DISTANCE BETWEEN 2
ADJACENT NUCLEI
SMB, Periodic Table Notes 2011 19
TREND GOING ACROSS A PERIOD
What is the ‘trend’ as you move left to right? ATOMIC
RADIUS DECREASES
Explanation: ---THE GREATER THE #PROTONS (NUCLEAR
CHARGE), THE STRONGER THE PULL ON THE E’S BRINGING
THEM CLOSER INTO THE NUCLEUS (SHIELDING)
SMB, Periodic Table Notes 2011 20
TREND GOING DOWN A GROUP OR FAMILY
What is the ‘trend’ as you move down a group? ATOMIC RADIUS INCREASES
Explanation: ----AS EACH ELEMENT GOES DOWN A GROUP,
YOU ADD ANOTHER NRG LEVEL INCREASING THE SHIELDING
SMB, Periodic Table Notes 2011 21
COMPARISON OF METALS TO NONMETALS
If you generally compare ionic size for metals and nonmetals, metal ionic sizes are SMALLER and nonmetal ionic sizes are BIGGER.
This is because metals tend to LOSE electrons and form CATIONS (and get smaller) while nonmetals tend to GAIN electrons and form ANIONS (and get larger).
SMB, Periodic Table Notes 2011 22
IONIZATION ENERGY (IE)
Description: AMOUNT OF ENERGY NEEDED TO REMOVE AN E- FROM AN ATOM. Atoms with a HIGH ionization energy
hold onto electrons MORE EASILY and are less likely to give them up.
Atoms with a LOW Ionization Energy hold onto electrons LOOSELY and are more likely to LOSE electrons
SMB, Periodic Table Notes 2011 23
TREND GOING ACROSS A PERIOD
What is the ‘trend’ as you move left to right? IE INCREASES Explanation: AS THE #PROTONS (AKA: NUCLEAR CHARGE)
INCREASES, THERE IS A GREATER PULL ON THE E’S REQUIRING MORE NRG TO REMOVE THEM
TREND GOING DOWN A GROUP OR FAMILY
What is the ‘trend’ as you move top to bottom? IE DECREASES
Explanation: Atom size increases making the outermost electron farther away from the nucleus therefore making it easier to remove
Shielding increases
1
2
3
4 5
6
7
INCREASES
DECREASES
SMB, Periodic Table Notes 2011 24
ELECTRONEGATIVITY (EN) Description: MEASURE OF AN ATOM’S ABILITY TO ATTRACT
ELECTRONS
Atoms with a HIGH Electronegativity have a STRONGER attraction for bonded electrons
Atoms with a LOW Electronegativity have a WEAKER attraction for bonded electrons
Based on a scale of 4, Fluorine has the greatest EN
SMB, Periodic Table Notes 2011 25
TREND ACROSS A PERIODWhat is the ‘trend’ as you move left to right? EN INCREASESExplanation: THERE ARE MORE PROTONS
(INCREASED ATOMIC NUMBER) WHICH
INCREASES THE ELECTRONS ATTRACTION
TREND GOING DOWN A GROUP OR FAMILY
What is the ‘trend’ as you move top to
bottom?
EN DECREASES
Explanation: AS YOU GO DOWN A GROUP
THERE ARE MORE ELECTRONS AND MORE NRG
LEVELS SO THE ATTRACTION GETS WEAKER
SMB, Periodic Table Notes 2011 26
Periodic Trends Summary(use reference Table S for data comparison)
TrendAcross a Across a period period
Down a Down a groupgroup
Ionization energy
increasesincreases decreasesdecreases
Electronegativity
increasesincreases decreasesdecreases
Atomic radii decreasesdecreases increasesincreases
Metallic properties
decreasesdecreases increasesincreases
Click on for video clip
SMB, Periodic Table Notes 2011 27
IV. Classification
Alkali MetalsAlkaline Earth MetalsTransition MetalsHalogensNoble Gases
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song
SMB, Periodic Table Notes 2011 28
Group 1: Alkali Metals
extremely reactive (not found free in nature)
form stable ionic compoundsreact with water to form a basereact with air to form oxidesreact with acids to form salts
Click on for video clip (2:56 min)
SMB, Periodic Table Notes 2011 29
Group 2: Alkaline Earth Metals
reactive (not found free in nature) - form stable ionic compounds
react with water to form a basereact with air to form oxides react with acids to form salts
Click on for video clip
SMB, Periodic Table Notes 2011 30
Groups 3-11: Transition Metals
multiple positive oxidation statesLose electrons from two outermost
energy levelsIons form colored solutions
Ex. CuSO4 (due to the Cu 2+ ion)
SMB, Periodic Table Notes 2011 31
Group 15 – unique features
Members range from typical nonmetals (nitrogen and phosphorus) through metalloids (arsenic and antimony) to metals (bismuth)
NitrogenForms stable diatomic molecules with a triple
bondComponent of proteinForms some unstable compounds that are used as
explosives
PhosphorusComponent of nucleic acids (DNA, RNA)More reactive than nitrogen at room temperature
SMB, Periodic Table Notes 2011 32
Group 16 – unique Features
Members range from typical nonmetals (oxygen and sulfur) through metalloids (selenium and tellurium) to metals (polonium)
Solids except oxygen Oxygen can exist as O2 and O3 (it is an allotrope)
Polonium is radioactive
SMB, Periodic Table Notes 2011 33
Group 17: Halogens
very reactive nonmetals - high electronegativity
not found free in natureform diatomic molecules when
freereact with metals to form salts
(halides)Found in all three phases (s, l,
g) due to differences in Van der Waals forces (these are weak)
SMB, Periodic Table Notes 2011 34
Group 18: Noble Gases
Have complete outer shellsAlmost inert (not reactive);
stableKrypton, xenon, and radon
form compounds with oxygen and fluorine
Referred to as monatomic gases
SMB, Periodic Table Notes 2011 35
TODAY……..TODAY……..
1. Using a pencil, transfer your RB answers to your scantron form –
In the green box, write “RB Topic 5 #1-45”.
Turn in BOTH the scantron and your written work.
SMB, Periodic Table Notes 2011 36
2. Assemble into NEW groups according to the number on your card from yesterday (refer to your sheet). Take your notes and 5 questions with you. Using your notes, discuss & complete the Teachback WS questions pertaining to your group.
Use the post-it notes for any questions you may have THAT MAY NEED ANSWERING
Folks who did the Noble gases will need to meet briefly for a few moments.
SMB, Periodic Table Notes 2011 37
3. Return BACK to your original groups and BEGIN your teachback. This NOT a silent lesson – use your “6 inch” voices to teach the other members. Ask your questions to ascertain clarity. At the end of this session, everyone in the group should have the Teachback WS completed.
Use the post-it notes for any questions you may have THAT NEED ANSWERING..
Once finished, begin RB questions 46-90.
Cooperation and diligence is necessary….. I will be watching and listening.
SMB, Periodic Table Notes 2011 38
TEACHBACK PROJECT REVIEW
Alkali MetalsAlkaline Earth MetalsTransition MetalsHalogensNoble Gases
Click for
song
SMB, Periodic Table Notes 2011 39
GROUP 1
1. The name of this group is ALKALI METALS
2. Does this group contain metals or nonmetals? METALS
3. Alkali metals (lose or gain)l LOSE electrons becoming (positive or negative) ions? POSITIVE
4. Describe the reactivity of the elements in this group as the atomic number increases. INCREASES
5. Are they (more or less) MORE reactive than all of the elements in Group 2 and why? THEY HAVE LOW IONIZATION ENERGIES
video
SMB, Periodic Table Notes 2011 40
Group 1 continued:
6. Can these compounds be found in nature in the elemental or combined state? COMBINED STATE IN THE FORM OF A SALT
7. What type of compounds do they normally form (ionic or covalent)? IONIC (M + NM)
8. If element Y represents an alkali metal, what is it’s general formula for the reaction with a:
Chloride: YCl Oxide: Y2O
9. What is the most reactive metal in this group? FRANCIUM
SMB, Periodic Table Notes 2011 41
GROUP 21. The name of this group is ALKALINE
EARTH METALS.
2. Does this group contain metals or nonmetals? METALS
3. They (lose or gain) LOSE electrons & form (positive or negative) ions POSITIVE ?
4. Describe the reactivity of the elements in this group as the atomic number increases (increases or decreases) DECREASES
5. Are they (more or less) LESS reactive than all of the elements in Group 1 and why? THEY HAVE GREATER IE
video
SMB, Periodic Table Notes 2011 42
Group 2 continued:6. Can these compounds be found in
nature in the elemental or combined state? COMBINED STATE IN THE FORM OF A SALT
7. What type of compounds do they normally form (ionic or covalent)? IONIC (M + NM)
8. If element Z represents an alkaline earth metal, what is it’s general formula for the reaction with a:
Chloride ZCl2 Oxide: ZO
SMB, Periodic Table Notes 2011 43
GROUP 151. What is this group referred to as? NITROGEN GROUP
2. Name the diatomic element in this group? NITROGEN
3. Classify each element in this group as a metal, non-metal or semi-metal (metalloid).
metals: ANTIMONY, BISMUTH nonmetals: NITROGEN, PHOSPHORUS semi-metal: ARSENIC
4. Explain what happens to the reactivity of a non-metal as the atomic number increases. DECREASES .
5. Which is the most reactive non-metal in this group? PHOSPHORUS
6. Is nitrogen a (diatomic or monatomic) DIATOMIC molecule & what type of bond is found in nitrogen? TRIPLE COVALENT
SMB, Periodic Table Notes 2011 44
GROUP 161. Classify each element in this group as a metal, non-metal
or semi-metal.metals: POLONIUM nonmetals: OXYGEN, SULFUR, SELENIUM semi-metal: TELLERIUM
2. Name the diatomic element in this group. OXYGEN
3. Define an allotrope? DIFFERENT FORMS OF AN ELEMENT IN THE SAME PHASE WITH HAVING DIFF CHEM & PHYSICAL PROPERTIES
4. Which element(s) in this group is an allotrope? SULFUR, OXYGEN (O2 and O3)
5. What type of element is Polonium? RADIOCATIVE METAL How can you tell it is radioactive? IT’S ATOMIC NUMBER IS GREATER THAN 83
SMB, Periodic Table Notes 2011 45
TRANSITION ELEMENTS (groups 3B-
12)
1.1. Which element is a liquid at room temperature? Which element is a liquid at room temperature? MERCURY (Hg)
2. What are the four main characteristic chemical 2. What are the four main characteristic chemical properties of transition elements? properties of transition elements?
MULTIPLE POSITIVE OXIDATION STATES IONS FORM COLORED SOLUTIONS LOSE ELECTRONS FROM TWO
OUTERMOST ENERGY LEVELS UNFILLED D ORBITALS
SMB, Periodic Table Notes 2011 46
GROUP 17
1. The name of this group is HALOGENS
2. Name and classify the elements in this group: METALS: At NONMETALS F, Cl, Br, I
3. Halogens (lose or gain) GAIN electrons becoming (positive or negative) ions? NEGATIVE
4. Why is astatine not included much in these discussions? NOT ENOUGH AVAILABLE TO STUDY
5. What would the general formula of a Group 17 element (represented by X) combined with magnesium of
group 2? MgX2
SMB, Periodic Table Notes 2011 47
6. What is the most reactive element in this group? FLUORINE
7. Can these compounds be found in nature in the elemental or combined state? COMBINED STATE AS SALTS
8. What type of salts do these elements form? HALIDES
9. For each state of matter, list the element(s) in this group. solid: IODINE liquid: BROMINE gas: CHLORINE, FLUORINE
10. What type of forces of attractions account for the different states of matter that exist and the high MP’s and BP’s as you go down the group? VAN DER WAALS FORCES (weak forces that get stronger as you go down the group )
SMB, Periodic Table Notes 2011 48
GROUP 18The name of this group is called NOBLE GASES.
What type of molecules do these gases form? (monatomic or diatomic) MONATOMIC
Describe the electron arrangement in the outermost energy level of all these elements. STABLE OCTECT – INERT GAS STRUCTURE
Which element has only two electrons? HELIUM
Describe the reactivity of the elements in this group. THEY ARE UNREACTIVE (Kr and Xe can be forced to react with F in lab settings)
SMB, Periodic Table Notes 2011 49
Topic 5 RB ANSWERS #46-90
71) _1_72) _3_73) _1_74) _2_
56) _2__
57) _3__
58) _3__
59) _2_
60) _1__
46) _2_
47) _1_
48) _4_
49) _1_
50) _1_
51)_ 2_
52) _4_
53)_4_
54) _3_
55) _2_
61) _3_
62) _3_
63) _1_
64) _1_
65) _3_
66) _1_
67) _2_
68) _2_
69) _4_
70) _1_
SMB, Periodic Table Notes 2011 50
79) They both follow the octet rule (8 valence e’s)
80) Bromine: MBr3 Oxygen: M2O3 Why? Group 13 has 3 valence e’s and will form a 3+ charge
81) Hydrogen is a NM & doens’t have the characteristics of other group 1 members other than one valence e
82) LARGEST: aluminum SMALLEST: carbon HIGHEST IE: carbon LOWEST IE: aluminum
83) Same number of valence e’s
84) Metals have fewer valence e’s. As you move to the right of the PT, there are more val e’s. Once the orbitals are full, a noble gas configuration is met (8 val e’s)
85) Metals become positive ions
87) MCl2 88) MgX2 89) X2O