Chemistry 11 Review

Group

Period

Family

Electronic configuration

Orbital

Long version

Short version

Atoms

Ions: cations & anions

XAZ

Valence Atomic charge

Periodic Trends

Atomic radius vs Electronegativity vs Electron affinity

Metals

Non Metals

Metalloids

Avogadro # = 6.02 x 1023

Diagonal rule

Balancing Equations

Types of Chemical Equations (S), (D), (SD), (DD), (CC), (IC)

STP / SATP

Mole Calculations

Stoechiometry

Common Ions (+) & (-)

Lewis DiagramBonding

% composition

Nomenclature

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1 IA

2 IIA

3 IIIB

4 IVB

5 VB

6 VIB

7 VIIB

8 VIIIB

9 VIIIB

10 VIIIB

11 IB

12 IIB

13 IIIA

14 IVA

15 VA

16 VIA

17 VIIA

18 VIIIA

Group New Version Old Version

Period

1

2

3

4

5

6

7

6

7

Family

Alkali metals

Alkaline earth metals

Metals of transition

Bo

ron

Fam

ily

Carb

on

Fam

ily

Nitro

gen

Fam

ily

Oxyg

en F

amily

Halo

gen

Fam

ily

No

ble G

as Fam

ily

Orbitals

pd

f

End of the electronic configuration

ELECTRONIC CONFIGURATION

s

Diagonal rule

1s1 1s2

2s1 2s2 2p1 2p2 2p3 2p4 2p5 2p6

3s1 3s2 3p1 3p2 3p3 3p4 3p5 3p6

4s1 4s2

Lantanide series

Actinides series

3d1 3d2 3d3 3d4 3d5 3d6 3d7 3d8 3d9 3d10 4p1 4p2 4p3 4p4 4p5 4p6

5s1 5s2 4d1 4d2 4d3 4d4 4d74d5 4d6 4d8 4d9 4d10 5p1 5p2 5p3 5p4 5p5 5p6

6s1 6s2 5d1 5d2 5d3 5d4 5d75d6 5d8 5d9 5d10

6d1 6d2 6d3 6d4 6d76d6 6d8 6d9 6d10

5d5

6d57s1 7s2

6p1 6p2 6p3 6p4 6p5 6p6

7p1 7p2 7p3 7p4 7p5 7p6

4f1 4f2 4f3 4f4 4f5 4f6 4f7 4f8 4f9 4f10 4f11 4f12 4f13 4f14

5f1 5f2 5f3 5f4 5f5 5f6 5f7 5f8 5f9 5f10 5f11 5f12 5f13 5f14

Metals

Non-Metals

Metalloids

Atoms vs Ions

Atomic

number

(Z)(p+)

Mass number

(A)(p++no)

proton

p+

neutron

no

electron

e-

Mg2412

Cl3517

12 12 12

22412Mg

12 24.3u

12 24.3u 12 12 10

Cl3517

17 35.45u 17 18 17

Cat+ions (+)

Anions (-)

17 35.45u 17 18 18

XAZ

Electronic Configuration Long version vs Short version and Ions

Long Version

20Ca: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2 since it has 20 e- and 20 exp.

20Ca2+: 1s2, 2s2, 2p6, 3s2, 3p6 since it has 18 e- and not 20 e-

53I: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10, 5p5

53I-: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10, 5p6

Short VersionPick the previous noble gas + …

20Ca: [Ar], 4s2

20Ca2+: [Ne], 3s2, 3p6

53I: [Kr], 5s2, 4d10, 5p5

53I-: [Kr], 5s2, 4d10, 5p6

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VALENCE ELECTRON: An electron that occupies the outermost energy level, or shell, of an atom.

ATOMIC CHARGE: The electric charge of an ion, equal to the number of electrons the atom has gained or lost.

VALENCE

CHARGE

1

1+2

2+

Most of the metal of transition have a valence of 2 which mean they would have a charge of 2+

3

3+

6

2-

5

3-

4

4+-

7

1-

2 or 8

0

Periodic TrendsAtomic radius: The distance from the centre of the nucleus to the outermost shell of an atom.

Periodic TrendsElectronegativity: A relative measure of an atom’s ability to attract the shared electrons in a chemical bond.

Periodic TrendsIonization Energy: the energy needed to remove electrons from an atom. Large atoms require low ionization energy while small atoms require high ionization energy.

Periodic Trends SUMMARY

This means that each human on earth has to eat 35000 eggs per second for 80 years?????? What about the # of chicken to produce that amount of eggs????

Avogadro # = 6.02 x 1023

How many eggs does each human on earth has to eat every second to add up to 1 mol in 80 years?

80 years x 365 day x 24 hours x 60 min. x 60 sec. = 2 522 880 00 s

Current earth population = 6 800 000 000 x 2 522 880 000 s = 1.72 x 1019 s

1 mole of eggs = 6.02 x 1023 eggs

6.02 x 1023 eggs = 35000 eggs / s

1.72 x 1019 s

1 year 1 day 1 hour 1 min.

Avogadro # = 6.02 x 1023

Avogadro’s Number:

1 mole of gas @ …

STP – Standard Temperature and Pressure:

V= 22.4L, 0ºC(273 K), 101.3 kPa

SATP – Standard Ambient Temperature Pressure

V= 24.8L, 25ºC(298 K), 101.3kPa

% Composition

• Percent Composition: The percentage, by mass, that each element that makes up a compound, out of 100%.

• To find the percent composition you must divide the mass of the element by the mass of the compound and multiply the result by 100.

• H2CO3 H x 2 = 2.0g/mol %H = 2/62 x 100 = 3.2%C x 1 = 12.0g/mol %C = 12/62 x 100 = 19.4%O x 3 = 48.0g/mol %O = 48/62 x 100 = 77.4%

Total = 62g/mol

1+ Charge 2+ Charge 3+ Charge 4+ Charge

Li+ Lithium Be2+ Beryllium Al3+ Aluminium Sn4+ Tin (IV)

Na+ Sodium Mg2+ Magnesium Cr3+ Chromium (III) Pb4+ Lead (IV)

K+ Potassium Ca2+ Calcium Fe3+ Iron (III)

Ag+ Silver Ba2+ Barium Au3+ Gold (III)

Cu+ Copper (I) Fe2+ Iron (II) Co3+ Cobalt (III)

NH4+ Ammonium Pb2+ Lead (II) Ni3+ Nickel (III)

H+ Hydrogen Ni2+ Nickel (II)

Zn2+ Zinc

Hg2+ Mercury (I)

Sn2+ Tin (II)

Co2+ Cobalt (II)

Cu2+ Copper (II)

Common Ions (+)

Common Ions (-)

Nomenclature

1. Magnesium Chlorate

2. Mercury II Chlorite

3. Lithium Sulfate

4. Zinc acetate

5. Sodium phosphide

4. Zinc acetate

5. Sodium phosphide

3. Lithium Sulfate

4. Zinc acetate

3. Lithium Sulfate

4. Zinc acetate

Mg(ClO3)2

Hg(ClO)2

Li2SO2

Zn(CH3CH2)2

Na3P

Nomenclature Game

Dimitry Vinagradov sofware

Bonding

A covalent bond is a form of chemical bonding that is characterized by the sharing of pairs of electrons between atoms, and other covalent bonds

You tube video: Covalent Bond

An ionic bond is a type of chemical bond formed through electrostatic attraction between two oppositely charged ions. Ionic bonds are formed between a metal and a nonmetal ion.

You tube video: Ionic Bond

Covalent Bonds

Covalent Bonds

What kind of bonds are theses? Song

Difference in Electronegativity

Lewis Symbols or Diagrams  Elemental properties and reactions are determined only by electrons in the outer energy levels. Electrons in completely filled energy levels are ignored when considering properties. Simplified Bohr diagrams which only consider electrons in outer energy levels are called Lewis Symbols. A Lewis Symbol consists of the element symbol surrounded by "dots" to represent the number of electrons in the outer energy level as represented by a Bohr Diagram. The number of electrons in the outer energy level is correlated by simply reading the Group number. Lewis symbols for oxygen, fluorine, and sodium are given in the diagram on the left. Lewis Symbols for the elements of the second period. Correlate the number of dots with the group number.

Balancing EquationsA chemical equation is an expression for a chemical reaction. It is a

quantitative statement indicating the number of moles of each reactant and of each product.

Reactants Products

In chemical equations, matter must be conserved. The number of atoms of each kind on the reactant side must equal those on the product side.

__Fe + __H2O → __Fe2O3 + __H22 3 3

__P4 + __Cl2 → __PCl346 DONE!

DONE!

__Fe2O3 + __CO → __CO2 + __Fe33 2 DONE!Σ R = Σ P

Types of Chemical EquationsSUMMARY

Let E= element and C = Compound

Reactants Reaction Type Products General Equation

E1 + E2 Combination (C) C R + S RS

C Decomposition (D) E1 + E2 RS R + S

E1 + C1 Single Displacement (SD)

E2 + C2 T + RS TS + R

C1 + C2 Double Displacement (DD)

C3 + C4 RS + TURU + TS

Hydrocarbon + O2

Complete Combustion (CC)

CO2 + H2O CH4+2O2 CO2+ 2H2O

Hydrocarbon + O2

Incomplete Combustion (IC)

CO + H2O 2CH4+3O2 2CO+ 4H2O

Stoichiometry

• is a branch of chemistry that deals with the quantitative relationships that exist between the reactants and products in chemical reactions.

• In a balanced chemical reaction, the relations among quantities of reactants and products typically form a ratio of whole numbers.

Mole Calculations

Mass – Mass: 2H2 + O2 2H2O

How many g of O2 is needed to burn with 10g H2?

10g H2 x 1 mol H2 x 1 mol O2 x 32g O2 =

2.02g H2 2 mol H2 1 mol O2

80g O2

Mole Calculations

Mass – Mol: 2KClO3 2KCl + 3O2

With 5g of KClO3, how many moles of KCl would you get?

5g KClO3 x 1mol KClO3 x 2 mol KCl =

122.45g KClO3 2 mol KClO3

0.041mol KCl

Mole Calculations

Mass – Molecules: 2H2 + O2 2H2O

How many molecules of O2 would you get if you start with 10g H2?

10g H2 x 1 mol H2 x 1 mol O2 x 6.02 x 1023 molecule O2 =

2.02g H2 2 mol H2 1 mol O2

1.5 x 1024 molecule O2

Mole Calculations

Mass – Volume: N2 + 3H2 2NH3

With 25g N2, find the volume of NH3 at STP

25g N2 x 1 mol N2 x 2 mol NH3 x 22.4L NH₃ =

28g N2 1 mol N2 1 mol NH3

40L NH3

Limited and Excessive Reactant

Limited Reactant (LR) – The substance in the formula that is used up first.

Excessive Reactant (ER) – The substance you have more of.

NH3 + HCl NH4Cl

What mass of ammonium chloride would you get if you add 1g NH₃ and 1g HCl?

1g NH3 = 0.0588 1g HCl = 0.0274

17g NH3 36.45g HCl

1.47g NH4Cl

HCl is your limited reactant since you get a smaller ratio. Therefore you get…

0.0274mol HCl x 1mol NH4Cl x 53.5g NH4Cl =

1 mol HCl 1 mol NH4Cl

This means that if you started with 1g HCl and it gave you 1.47 g of NH4Cl you can conclude that you used 0.47g of NH3 therefore since we started with 1g of NH3 we know that we have 0.53 g extra.

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