PassGAMSAT Science EClass 2 Exercise

PassGAMSAT Science eClass 2 Exercises

eClass 2 Exercises 1. Write the names for these ionic compounds: Compound formula

Compound name

NaHCO3

sodium bicarbonate

CaCO3

calcium carbonate

NH4NO3

ammonium nitrate

Cu2SO4

Copper (I) sulfate

AgNO3

silver nitrate

KI

potassium iodide

2. Write Lewis electron dot structures for these compounds: Compound name

Compound formula

ammonia

NH3

hydrochloric acid

HCl

carbon dioxide

CO2

carbon tetrachloride

CCl4

Lewis dot structure

H NH H H Cl O C O Cl Cl C Cl Cl

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3. Name these covalent compounds:

Compound formula

Compound name

CF4

carbon tetrafluoride

PCl3

phosphorus trichloride

SF6

sulfur hexafluoride

H2S

hydrogen sulfide

4. Write the formulas for these compounds:

Compound name

Compound formula

hydrogen bromide

HBr

silicon dioxide

SiO2

oxygen dichloride

OCl2

silicon tetrahydride

SiH4

5. Calculate the formula weight for these compounds, then the weight of one mole of each:

Compound formula Formula weight

Weight of 1 mole

Ba(NO3)2

261.3

261.3 g

FeSO4

151.92

151.92 g

H2O2

34.02

34.02 g

CH3NH2

31.07

31.07 g

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6. What is the mass in grams of each of the following elements or compounds?

Quantity of substance

Mass in grams

2.00 moles of N2

56.04 g

15.8 moles of SO2

1012.208 g

1 mole of LiCl

42.394 g

1.86 moles of Au

366.36 g

7. What is the mass percent of each element in the compound NH 4NO2? nitrogen, 43.7%; hydrogen 6.3%; oxygen 50%

8. Write a balanced equation to describe this reaction: sulfur dioxide gas reacts with oxygen gas to produce sulfur trioxide. 2SO2(g) + O2(g) → 2SO3 (g)

9. Balance this equation: H2SO4 + KOH → H2O + K2SO4 H2SO4 + 2KOH → 2H2O + K2SO4

10. Calculate the molarity of each of these solutions:

Solution

Molarity

3.0 liters of solution containing 120 g of

0.67M

acetic acid (C2H3O2H) 20 g NaOH in 500 ml of solution

1M

1 mole of solute in 500 ml of solution

2M

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11. Calculate the mass in grams of solute needed for these solutions: Solution

Grams of solute

1 L of 0.5M NaOH

20

100 ml of 1M KCl

7.45

1 L of 0.3M NaCl

17.53

2 L of 0.1M glucose (C6H12O6)

36

12. What type of reaction is each of the following? Reaction

Type

2KClO3→ 3O2 + 2KCl

decomposition

ZnO + H2 → Zn + H2O

displacement

CaO + CO2 → CaCO3

combination

H2SO4 + 2KOH → 2H2O + K2SO4

double displacement

13. What is the oxidation number for the colored element in each of these compounds? Compound

Oxidation number

CH4

-4

P4

0

CaCO3

4

MnCl2

2

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14. Determine whether each of the following reactions is a redox reaction. Reaction

Redox

4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)

X

Not redox

X

NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) Cl2(g) + H2O(l) → HCl(aq) + HClO(aq)

X

3As2O3 + 7H2O + 4NO3- + 4 H+↔ 6H3AsO4 + 4NO

X

15. In each of the following reactions, determine which reactant is the oxidizing agent and which is the reducing agent. Reaction

Oxidizing agent

Reducing agent

2Mg + O2→ 2MgO

O2

Mg

Mg + Cl2→ MgCl2

Cl2

Mg

Sn + F2→ SnF2

F2

Sn

ZnO + H2→ Zn + H2O

ZnO

H2

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