Elements and compounds in our surroundings

Chemistry I

Stage II

Ms. Claudia Barahona

Elements & compounds

in our surroundings

Stage I1

Chemical reactions in our

surroundings

Formative Objective: The student

identifies the chemical name and formula of

elements and compounds present in our

daily lives, to reflect on the effects and

importance of these substances in our

bodies and surroundings.

Elaborated by: QFB. Claudia Barahona

TOPICS

Classification of elements in : metals,

nonmetals and metalloids

Classification of compounds by the number of

elements and chemical function.

Elements present in the human body and

acquisition sources.

The effects and uses of chemical compounds

in our daily lives

COMPETENCES

Generic Competences:

4. Listens, interprets, and emits pertinent messages in different situations using mediums, codes and appropriate tools.

Express ideas and concepts through

Identifies the main ideas in a text or an oral speech, and deduce conclusions from them.

5. Develops innovations and proposes solutions from established methods.

Follows directions and procedures objective.

Synthesizes evidences obtained with experimentation to produce

Uses the information and communication technologies to

Disciplinary Competences:

2. The student bases opinions about the impact of science and technology in his daily life assuming ethical considerations.

10. The Student relates the symbolic expressions of a phenomenon of the sight or using scientific instruments or models.

Activity 2.1

Exploring your knowledge

What is an ELEMENT?

o A pure substance

composed of only one

type of atom.

o Cannot be broken

down into another

substance by chemical or

physical means.

Compounds

A pure substance consisting of 2 or more elements chemically combined, in a definite composition that can be broken down into a simpler substance, using chemical methods of separation.

Chemical methods:

◦ Electrolysis

◦ REDOX reactions

◦ Catalysis

Dmitri Mendeleev (1869)

http://www.chem.msu.su/eng/misc/mendeleev/welcome.html

The periodic table

Arrangement of elements by increasing

atomic number

http://www.chem.msu.su/eng/misc/mendeleev/welcome.html

Act 2.1 Q 4

Representative

elements

Transition

Metals

Chemical Symbols

Are one or two-letter abbreviations for the

names of an element.

ONLY THE FIRST LETTER IS CAPITALIZED.

If the symbol has a second letter, it is lowercase

SO THAT WE KNOW WHEN A DIFFERENT

ELEMENT IS INDICATED.

CARBON MONOXIDE Cobalt

The symbol of Carbon is C, the symbol of sulfur

S. However the symbol of Cesium is Cs not CS.

Why not?

Origin of some of the elements

Most of the chemical symbols use

letters from the current name, some

are derived from their ancient name.

Other elements are named after

planets, mythological figures, colors,

minerals, geographical location and

famous people.

Act 2.1

Part II

Activity 2.2 Acquisition of knowledge

Vocabulary terms

1. Periodic table

2. Period

3. Group or family

4. Chemical symbols

5. Representative elements

6. Transition elements

7. Metals

8. Nonmetals

9. Metalloids

10. Malleable

11. Ductile

12. Element

13. Compound

14. Binary compound

15. Ternary compound

16. Polyatomic compound

17. Acids

18. Bases

19. Oxides

20. Salts

21. Valence electrons

22. Ionic bond

23. Covalent bond

Typical amounts of essential

elements in:

Planet

Universe

Act 2.2 Part III Element Real case

intoxication

(lethal dose)

Source of acquisition Symptoms First aid in case of

intoxication

Arsenic (As)

Can be administered

through oral via such as

food, drinks, etc.

In adults is estimated to

be 70 to 200 mg or

1 mg/kg/day.

Headaches,

confusion,

severe diarrhea,

drowsiness.

Convulsions.

vomiting, blood

in the urine,

cramping

muscles, hair

loss, stomach

pain, and more

convulsions. The

final result of

arsenic

poisoning is

coma and

death.

Dimercaproland dimer

captosuccinic

acid are chelating

agents that sequester

the arsenic away from

blood proteins.

Act 2.2 Part III

Element Real case

intoxication

(lethal dose)

intoxication

Chromium (Cr)

Drinking water,

Ranges between 1900

and 3300 µg/kg.

Chromate dye company.

Cr often used to

manufacture, amongst

other things, leather

products, paints, cement,

mortar and anti-

corrosives.

Can lead

to DNA

damage. After it

reaches the

blood stream, it

damages

kidneys, liver

and blood cells,

Hemolysis, rena

l and liver

failure are the

results of these

damages.

Appropriate supportive

measures may include

ventilatory support,

cardiovascular support,

and renal and hepatic

function monitoring.

Check the 7 diatomic molecules

Act 2.2 Part III Element Real case

intoxication

(lethal dose)

intoxication

Mercury

Consumption of fish is

by far the most

significant source of

ingestion-related

mercury exposure in

humans and animals,

although plants and

livestock also contain

mercury due

to bioconcentration of

mercury from seawater,

freshwater, marine and

lacustrine sediments,

soils.

Sensory

impairment

(vision, hearing,

speech),

disturbed

sensation and a

lack of

coordination.

Damage to the

brain, kidneys

and lungs

Immediate chelation

therapy,

Check the 7 diatomic molecules

The Periodic Table

A map of the building block of matter.

18VIIIA

1.00797

Periodic Table 13IIIA

17VIIA

4.0026

Li6.939

9.0122

10.811

12.0112

14.0067

15.9994

18.9984

20.179

Na22.9898

12Mg24.305

8 9VIIIB

10 11IB

26.9815

28.086

30.9738

32.064

35.453

39.948

39.102

20Ca40.08

44.956

50.942

51.996

54.9380

55.847

58.9332

28Ni58.71

29Cu63.54

30Zn65.37

31Ga65.37

32Ge72.59

74.9216

34Se78.96

79.909

36Kr83.80

Rb85.47

38Sr87.62

88.905

40Zr91.22

92.906

42Mo95.94

43Tc[99]

101.07

102.905

46Pd106.4

107.870

112.40

114.82

118.69

121.75

127.60

126.904

131.30

132.905

137.34

138.91

178.49

180.948

183.85

75Re186.2

76Os190.2

195.09

196.967

80Hg200.59

204.37

207.19

208.980

84Po[210]

85At[210]

86Rn[222]

787Fr[223]

88Ra[226]

89Ac[227]

104Ku[260]

105 106 107 108 109http://www.chemsoc.org/viselements/pages/periodic_table.html

Reading the Periodic Table: Classification

Nonmetals, Metals, Metalloids, Noble gases

Across the Periodic Table Periods: Are arranged horizontally across the

periodic table (rows 1-7) These elements have the same number of valence shells.

18VIIIA

IIIA14

IVA15VA

17VIIA

VIIB8 9

VIIIB10 11

IB12IIB

2nd Period

6th Period

Down the Periodic Table Family: Are arranged vertically down the periodic table (columns or group, 1- 18 or 1-8 A,B)

These elements have the same number electrons in the outer most shells, the valence shell.

18VIIIA

IIIA14

IVA15VA

17VIIA

VIIB8 9

VIIIB10 11

IB12IIB

Alkali Family:

1 e- in the valence shell

Halogen Family:

7 e- in the valence shell

Infamous Families of the Periodic Table

Notable families of the Periodic Table and some important members:

18VIIIA

IIIA14

IVA15VA

17VIIA

VIIB8 9

VIIIB10 11

IB12IIB

Alkali

Alkaline

(earth)

Transition Metals

Noble Gas Halogen

Chalcogens

Classification of Elements

Metals

Metals appear to the left of the dark ziz-zag line

on the periodic table. Most metals are solid at room temperature.

Properties of metals

Metals have

luster. This

means they are

Ductile metals can be

drawn into wire.

COPPER

Malleable

metals can

be hammered

into sheets

ALUMINUM

Metals have a high melting point. They

are also very dense.

Conductors

Metals are

conductors of electricity and

A chemical property

of metal is its

reaction with

water and oxygen.

This results in

corrosion and

• Shiny

• Solids at room T° (except Hg)

• Luster

• Good conductors of heat and electricity

• Malleable (sheet)

• Ductile (wires)

• High melting points

• High density

Non-metals

Nonmetals occur to the right of the dark zig-zag on the periodic table. Although Hydrogen is in family 1, it

is also a nonmetal. Many nonmetals are gases at room temperature.

Properties of Non metals

Nonmetals do

not have

luster; they are dull.

Properties of Non-metals

Brittle Nonmetals are

brittle so they

break easily. This means nonmetals ARE NOT ductile or

malleable.

Nonmetals

have low

density.

They also have a low melting point. This is why they are poor conductors of

heat and electricity.

Properties of nonmetals

Nonmetals:

Lacks of luster

Low melting point

Low density

Bad conductors of heat or electricity

Metalloids

Metalloids can be found clustered around the

dark zig-zag line that separates metals and

nonmetals.

Properties of Metalloids

Metalloids (metal-

like) have

properties of both

metals and

nonmetals.

Metalloids are solids

that can be

shiny or dull.

They conduct

electricity and

heat better than

nonmetals but not

as well as metals.

Metalloids are

malleable and

ductile

Properties of metals, nonmetals and

metalloids Metalloids:

Possess characteristics of both metals and

nonmetals

Semiconductors

Summary

What is a COMPOUND?

o A substance in

which two or

more different

elements are

CHEMICALLY

bonded together.

Types of Compounds

• A compound with 2 different elements

• NaCl – Sodium Chloride Binary

• A compound with 3 different elements

• HClO Hypochlorous Acid Ternary

• A compound with 3 or more elements

• NaHCO3 Sodium Bicarbonate

Polyatomic

Classification of Inorganic

Compounds

INORGANIC

COMPOUND

CLASSIFICATION

ELEMENTS Metal

Non-metals

Metalloids

COMPOUND Salt

Others*

Contain the H+ ion and a non-metal ion or

polyatomic ion in an aqueous (aq) solution

CATION ANION

HCl -> Hydrochloric acid

H2SO4 -> Sulfuric acid

Some characteristics

Taste Sour

Feel May Sting

Litmus Red

Phenolphthalein Colorless

Neutralization Neutralizes bases

Strong acids

6 common strong acids:

• Perchloric acid

• Sulfuric acid

• Hydroiodic acid

• Hydrobromic acid

• Hydrochloric acid

• Nitric acid

Contain a metal ion and the (OH)- ion in an

aqueous (aq) solution

CATION ANION

Characteristics of bases

Taste Bitter, chalky

Feel Soapy, slippery

Litmus Blue

Phenolphthalein Pink

Neutralization Neutralizes acids

No special naming rules for bases.

Ex. KOH -> potassium hydroxide

Ex. NH4OH -> ammonium hydroxide

OXIDES

Binary compounds that contain a metal or

non metal ion and the O-2 ion, normally in a

solid state (s)

Al2O3 is aluminum oxide ( Ionic M-NM)

CO carbon monoxide (Covalent NM-NM)

Contain a metal ion (Not H+) and non-metal ion or

polyatomic ion (NOT (OH)- nor, O-2 )

1. normally in a solid state, (s), or in an aqueous, (aq),

solution

2. SALTS ARE FORMED AFTER THE NEUTRALIZATION

OF AN ACID BY A BASE

Example:

LiF lithium fluoride

MgCr2O7 magnesium dichromate

Pb(ClO3)4 lead (IV) chlorite

CATION ANION

Others

Ionic compounds

Covalent compounds

Ionic compounds

Ions are held together by strong electrical attractions between the opposite charges called ionic bonds. ◦ Cation= Metal

◦ Anion= Nonmetal

The sum of the ionic charges

on the formula is always

zero!!

CATION ANION

Covalent compounds

Forms when atoms of 2 nonmetals share electrons.

Held together by the sharing of electrons called covalent bond.

When 2 or ore atoms share electrons they form a molecule.

CATION ANION

Review

Classify the following compounds based on the number of elements and function.

1. AgOH

2. MgO

3. KOH

4. CaF2

5. Na2CO3

6. Na3PO4

7. CaCO3

8. H2SO4

9. ClO3

10. SO3

11. Fe203

12. Mg(OH)2

13. HNO3

14. PbO2

15. CO2

16. Na2O

17. HBr

Activity 2.4

Elements in their natural state

Simplest kind of pure substance that contains only one

type of matter and cannot be broken down by chemical

methods.

Most of the elements in their natural state are

found as compounds.

Diatomic molecules

7 elements are found as diatomic molecules:

◦ H2, N2, O2, F2, Cl2, Br2 e I2

Chemical compounds by

number of

elements

Compounds

Two or more elements chemically combined.

Number of elements

Compounds can be classified according to

the number of different elements

chemically combined as:

◦ Binary (two elements)

Ex: NaCl, FeS, H2O.

◦ Ternary (Three elements)

Ex: NaOH, HClO4, H2SO4

◦ Polyatomic (four or more)

Ex: NaHCO3, (NH4)2SO4, NaHSO3

Classification of compounds by their

function

compounds

Acids Bases Oxides Salts

Acids and bases

Lemons

Grapefruits

Vinegar

Sodium hydroxide

Antiacids

Acetic acid

Arrhenius theory: Substance that dissolves in

water and produces hydrogen ions (H+).

Bronsted-Lowry: Proton donor substances.

Properties of Acids

Sour taste.

Turns litmus paper indicator red.

Turns phenolphtalein indicator colorless.

Corrode some metals.

Arrhenius theory: Substance that dissolves in

water and produces hydroxide ions (OH-).

Bronsted-Lowry: Proton acceptor substances.

Properties of Bases

Bitter taste.

Slippery feel (soaps).

Turns litmus indicator blue.

Turns phenolfphtalein indicator pink.

Oxides

Chemical binary compounds with one or

more oxygen atoms combined with another

element.

Ionic compound that contains a metal ion or

NH4+ and a nonmetal or polyatomic ion

other than OH-.

Chemical compounds by

type of bond

Ionic compounds

Consists of positive ion (metal) and negative ion

(nonmetal).

Metal - Nonmetal

Ions are held together by strong electrical

attractions between the opposite charges called

ionic bonds.

Covalent compounds

Forms when atoms of 2 nonmetals share

electrons.

Nonmetal – Nonmetal

Held together by the sharing of electrons called

covalent bond.

When 2 or more atoms share electrons they

form a molecule.

Electronegativity

Relative ability of an atom to attract the

share electrons by itself.

In a period, it increases.

In a group it decreases.

Nonmetals, Fluorine 4.0 and oxygen 3.5

have the highest electronegativites.

Metals Cesium and Francium have the

lowest electronegativities.

Electronegativity

Increasing electronegativity

Representative

elements

Transition

Metals

Polarity

• Describes how electrons are shared between

atoms .

• Electrons are not always shared equally

between two bonding atoms.

• One atom might exert more of a force on the

electron than the other, electronegativity.

• The unequal sharing of electrons within a bond

leads to the formation of polarity.

Polarity of bonds

Nonpolar covalent bond: Bond between

atoms with identical or very similar

electronegativities.

Polarity of bonds

Polar covalent bond: Electrons are shared

unequally.

Summary of bonds

Topic: Chemical elements and compounds in your body and surroundings

Compound Formula Elements

involved

Classificatio

n by # of E

Classification

by chemical

function

Carbon dioxide CO2 Carbon

Oxygen

Binary Oxide

Hydrochloric acid HCl Hydrogen

Chlorine

Binary Acid

Vinegar (Acetic

CH3(COOH) Carbon

Hydrogen

Oxygen

Ternary Acid

Table salt

(sodium chloride)

NaCl Sodium

Chlorine

Binary Salt

Topic: Chemical elements and compounds in your body and surroundings

Compound Formula Elements

involved

Classificatio

n by # of E

Classification

by chemical

function

Sodium

bicarbonate

NaHCO3 Sodium

Hydrogen

Carbon

Oxygen

Polyatomic Salt

Sodium hydroxide NaOH Sodium

Oxygen

Hydrogen

Ternary Base

Calcium oxide CaO Calcium

Oxygen

Binary Oxide

Nitrogen

monoxide

NO Nitrogen

Oxygen

Binary Oxide

1. An ionic compound is a chemical compound in

which ions are held together by the electrostatic

force between oppositely charged ions.

2. An ionic compound is form by a positively charge ion

called a cation, which is always a metal and a

negatively charged ion called a anion which is always

a nonmetal or a polyatomic ion when we have 2

or more nonmetals together with a charge.

3. The main difference between ionic and covalent

compounds is that ionic compounds is composed of

a metal bonded to a nonmetal while a covalent

compound is a nonmetal bonded to a nonmetal.

4. In ionic compounds there is a complete

transference of electrons.

5. In covalent compounds electrons are being shared.

Compound Classification Compound Classification

BaCl2 Ionic Cl2O covalent

N2O4 Covalent KF Ionic

Compounds according to the type of

Ionic compounds

Consists of positive ion (metal) and negative ion

(nonmetal).

Ions are held together by strong electrical

attractions between the opposite charges called

ionic bonds.

Covalent compounds

Forms when atoms of 2 nonmetals share

electrons.

Held together by the sharing of electrons called

covalent bond.

When 2 or more atoms share electrons they

form a molecule.

Metallic bonds

Bonding of atoms in solid metallic

crystals.

A three-dimensional array of positive ions

that remain fixed in the crystal lattice

while loosely held valence electrons move

freely throughuot the crystal.

Sharing a “sea of ve-”.

e- are free to move.

Properties

Good conductors of electricity and heat

Insoluble in water

Malleable (sheets)

Ductile (wires)

END OF STAGE 2

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