Second Semester Chemistry Review

2.78 km to cm

278,000

3389 micrograms to grams

0.003389 grams

9.358 × 10² nm to km

9.358 × 10^-4

83.832 L to mL

83832 mL

515 ms to cs

51.5

35 MHz to Hz

3.5 × 10^-5

Definition of cation

Positively charged ion

Definition of anion

Negatively charged ionm

Polyatomic ion

Charged combined ions

How are atoms held together?

Opposite attraction

What are ionic compounds characteristics?

Hard, brittle, high melting points

How do you know if a compound is covalent?

If it is metal + nonmetal

When do you use prefixes?

When you need to specify # of atoms of an element

What is the octect rule?

All shells need 8 electrons

What does “binary” mean? Give an example of a binary ionic compound

Binary means something of two parts. A binary ionic compound is a chemical substance made of two different elements: a positively charged metal and a negatively charged nonmetal

When do you use a roman numeral?

When you have transition metals

What elements are transition metals but do not require roman numerals? Why do they not need them?

Silver, Zinc, Cadmium. They form one stable charge.

What is the most common charge for group 1?

+1

What is the most common charge for group 2?

+2

What is the most common charge for group 13?

+3

What is the most common charge for group 15

-3

What is the most common charge for group 16

-2

What is the most common charge for group 17?

-1

List some of the properties that are affected by intermolecular forces:

They affect boiling points, solubility, viscosity, surface tension, and density (there’s likely much more, but this is what I found on google).

What are the four intermolecular forces and what type of compound has that main force?

Hydrogen bonding, affects compounds of hydrogen that are bonded to either nitrogen, oxygen, or fluorine.
Dipole Dipole, polar covalent compounds.
Ion-bonding, solutions that contain both ionic and polar molecules.
London dispersion force, nonpolar covalent compounds.

Rank the intermolecular forces from weakest to strongest:

1. London dispersion forces

2. Dipole-Dipole

3. Hydrogen bonding

4. Ion-Dipole forces

List the following substances in order of increasing intermolecular forces: H2, NF3, O2, C3H8, H2O, CO2

H2, O2, CO2, C3H8, NF3, H2O

Write the ten prefixes used for molecular compounds:

1. Mono

2. Di

3. Tri

4. Tetra

5. Penta

6. Hexa

7. Hepta

8. Octa

9. Nona

10. Deca

What is this compounds name: Mg

Magnesium

What is this compounds name: SO4

Sulfate tetraoxide (this is sulfate but this the name before that is the one that takes prefixes into account).

What is this compounds name: Cl2O3

Trichloride trioxide

What is this compounds name: NBr3

Nitrogen tribromide

What is this compounds name: PBr5

Phosphate pentabromide

What is this compounds name: Cl2O

Dichloride monoxide

What is this compounds name: IF7

Iodine heptafluoride

What is this compounds name: KCL

Potassium monochloride

What is this compounds name: Na2CO3

Sodium carbonate

What is this compounds name: CuSO4

Copper sulfate

What is this compounds name: ZnO

Zinc oxide (no prefixes needed, metal to nonmetal)

What is this compounds name: Fe2O3

Iron(III) oxide

What is this compounds name: Pb(ClO2)2

Lead(II) Chlorite

What is this compounds name: Al2(SO4)3

Aluminum sulfate

What is this compounds name: FeCl3

Iron (III) Chloride

What is this compounds name: PbSO4

Lead (II) Sulfate

Write the formula for the following compound: ammonium sulfade

(NH₄)₂SO₄ (just realized I can do subscripts but im not changing allat ngl)

Write the formula for the following compound: sodium nitrate

Na(NO₃)

Write the formula for the following compound: lead(II) chlorite

Pb(ClO₂)₂

Write the formula for the following compound: potassium nitrate

K(NO₃)

Write the formula for the following compound: iron(II) sulfite

Fe(SO₃)

Write the formula for the following compound: magnesium nitrate

Mg(NO₃)₂

Write the formula for the following compound: lead(II) phosphate

Pb₃(PO₄)₂

Write the formula for the following compound: iron(III) chromate

Fe₂(CrO₄)₃

Write the formula for the following compound: diphosphorus pentoxide

P₂O₅

Write the formula for the following compound: copper (I) hydroxide

CuOHW

Write the formula for the following compound: copper(II) hydroxide

Cu(OH)₂

Write the formula for the following compound: nickel (II) nitrate

Ni(NO₃)₂

Write the formula for the following compound: silver cyanide

AgCN

Do the following for this equation: Balance, identify the reaction type, and complete the mole ratio problem for each reaction. Here is your equation: SiCl₄ + H₂O → SiO₂ + HCl

Here’s your problem: If 3.4 moles of silicon tetrachloride are used in the above reaction, how many moles of hydrogen chloride will be produced?

1. Balanced equation: 1 SiCl₄ + 2 H₂O → 1 SiO₂ + 4 HCl

2. Reaction type: Double replacement

3. 3.4 × 4 mol HCl / 1 mol SiCl₄, so 13.6

Do the following for this equation: Balance, identify the reaction type, and complete the mole ratio problem for each reaction. Here is your equation: P + NaOH → Na₃PO₃ + H₂

Here’s your problem: When 4.5 moles of hydrogen gas are created in the above reaction, how many moles of phosphorus were used?

1. Balanced equation: 2P + 6NaOH → 2Na₃PO₃ + 3H₂

2. Single replacement

3. 4.5 × 2/3 = 3

Do the following for this equation: Balance, identify the reaction type, and complete the mole ratio problem for each reaction. Here is your equation: N₂ + O₂ + H₂O → HNO₃

Here’s your problem: How many moles of nitric acid (HNO₃) are created when 9.7 moles of nitrogen are used in excess oxygen and water?

1. Balanced equation: 2N₂ + 5O₂ + 2H₂O → 4HNO₃

2. Synthesis

3. 9.7 × 4/2 = 19.4

Do the following for this equation: Balance, identify the reaction type, and complete the mole ratio problem for each reaction. Here is your equation: C₅H₈ + O₂ → CO₂ + H₂O

Here’s your problem: In a reaction where pentyne reacts with oxygen to produce 43 moles of water, how many moles of carbon dioxide are also produced?

1. Balanced equation: C₅H₈ + 7O₂ → 5CO₂ + 4H₂O

2. Combustion

3. 43 × 5/4 = 53.75

Do the following for this equation: Balance, identify the reaction type, and complete the mole ratio problem for each reaction. Here is your equation: NH₄NO₃ → N₂ + O₂ + H₂O

Here’s your problem: If 8.2 moles of ammonium nitrate decompose, how many moles of oxygen gas are produced?

1. Balanced equation: 2NH₄NO₃ → 2N₂ + O₂ + 4H₂O

2. Decomposition

3. 8.2 × ½ = 4.1

Do the following for this equation: Balance, identify the reaction type, and complete the mole ratio problem for each reaction. Here is your equation: Na₃As + F₂ → NaF + As

Here’s your problem: How many moles of arsenic are created when 6.7 moles of sodium arsenic react with excess fluorine?

1. Balanced equation: 2Na₃As + 3F₂ → 6NaF + 2As

2. Single replacement

3. 6.7 × 2/2 = 6.7

Change each word equation into a formula equation, then indicate the reaction type: When heated solid potassium hydroxide turns into solid potassium oxide and steam

2KOH (s) → K (s) + H₂O (g), decomposition

Change each word equation into a formula equation, then indicate the reaction type: A silver iodide precipitate and aqueous sodium nitrate form when a silver nitrate solution and a sodium iodide solution react

AgNO₃ (aq) + NaI (aq) -. AgI (s) + NaNO₃ (aq), double replacement

Change each word equation into a formula equation, then indicate the reaction type: When liquid octanol (C₈H₁₇OH) is burned in oxygen gas, carbon dioxide gas and water vapor are produced

C₈H₁₇OH(l) + 12O₂ (g) → 8CO₂ (g) + 9H₂O (g), combustion

Change each word equation into a formula equation, then indicate the reaction type: The solid blue green copper (II) oxide that covers the statue of liberty is created when the copper metal is exposed to oxygen gas over a long period of time

2Cu (s) + O₂ (g) → 2CuO (s), synthesis

Change each word equation into a formula equation, then indicate the reaction type: The hydrogen sulfate solution in a car battery reacts with the lead plates in it to create a lead (II) sulfate solution and hydrogen gas

Pb (s) + H₂SO₄ (aq) → PbSO₄ (aq) + H₂ (g), single-replacement

First, change the word formula equation into a word equation, then balance it, and then indicate the reaction type. Here is your formula: P₄O₁₀ → P + O₂

1. Tetraphosphorus decaoxide decomposes into phosphorus and oxygen gas

2. P₄O₁₀ → 4P + 5O₂

3. Decomposition

First, change the word formula equation into a word equation, then balance it, and then indicate the reaction type. Here is your formula: C₁₂H₂₂O₁₁ (sucrose) + O₂ → CO₂ + H₂O

1. Sucrose and oxygen gas react to create carbon dioxide and water

2. C₁₂H₂₂O₁₁ + 12O₂ → 12CO₂ + 11H₂O

3. Combustion

First, change the word formula equation into a word equation, then balance it, and then indicate the reaction type. Here is your formula: Ca₃N₂ + SnF₄ → CaF₂ + Sn₃N₄

1. Calcium Nitride reacts with tin (IV) fluoride to produce Calcium Fluoride and Tin (IV) nitride

2. Ca₃N₂ + SnF₄ → CaF₂ + Sn₃N₄

3. Double replacement

First, change the word formula equation into a word equation, then balance it, and then indicate the reaction type. Here is your formula: W + Cl₂ → WCl₅

1. Tungsten reacts with chloride to synthesize tungsten (V) chloride

2. 2W + 5Cl₂ → 2WCl₅

3. Synthesis

First, change the word formula equation into a word equation, then balance it, and then indicate the reaction type. Here is your formula: Li + Au(NO₃)₃ → LiNO₃ + Au

1. Lithium reacts with gold (III) nitrate to produce lithium nitrate and gold

2. Li + Au(NO₃)₃ → LiNO₃ + Au

3. Single replacement

With the given equation, balance it and perform a given calculation:

KCl + AgNO₃ → KNO₃ + AgCl
Given 0.5 moles of silver chloride, calculate the number of particles of silver nitrate

1. KCl + AgNO₃ → KNO₃ + AgCl

2. 0.5 × 1/1 × 6.022e23, 3.011e23

With the given equation, balance it and perform a given calculation:

Al + CuCl₂ → AlCl₃ + Cu

Given 15.2 g of copper (II) chloride, calculate the number of moles of aluminum chloride

1. 2Al + 2CuCl₂ → 2AlCl₃ + 2Cu

2. 15.2 × 1/134.45 × 2/3, 0.0754 moles

With the given equation, balance it and perform a given calculation:

Pb(NO₃)₂ + K₂S → PbS + KNO₃

Given 10.5 g of KNO₃, calculate the number of grams of K₂S

1. Pb(NO₃)₂ + K₂S → PbS + 2KNO₃

2. 10.5 × 1/101.11 × ½ * 110.26/1 = 5.72 g

For the reaction CS₂ + O₂ → CO₂ + SO₂, how many grams of oxygen are needed to produce 6 moles of sulfur dioxide?

1. Balance, so CS₂ + 3O₂ → CO₂ + 2SO₂

2. 6 × 3/2 × 32 = 288 g

For the reaction HgO → Hg + O₂, how many molecules of oxygen are produced from the decomposition of 100 grams of mercury (II) oxide?

1. Balance the equation, so 2HgO → 2Hg + O₂

2. 100 × 1/216.59 × ½ * 6.022e23

3. 1.39e23

For the reaction H₂ + O₂ → H₂O, how many grams of water are produced from 64 g of oxygen? If 65 g of water are produced in the lab, what is the percent yield?

1. Balance, so 2H₂ + O₂ → 2H₂O

2. Theoretical yield: 64 × ½ 2/1 18.02 = 72.08

3. (65×72.08) * 100

4. 90.2 %

Identify the limiting and excess reactant when 1.22 g of O₂ reacts with 1.05 g of H₂ to produce water.
Formula: 2H₂ + O₂ → 2H₂O

1. 22 × 1/32 × 2/1 × 18.02 = 1.37

2. 1.05 × 1/2.02 × 2/2 × 18.02 = 9.37

3. ER: 9.37 LR 1.37

Identify the limiting and excess reactant when 24.68 g of CS₂ reacts with 2.88 g of O₂ to produce CO₂ and SO₂
Formula: CS₂ + 3O₂ → CO₂ + 2SO₂

1. 2.88 × 1/32 × 1/3 = 0.0300 CO₂

2. 24.68 × 1/76.13 × 1/1 = 0.324 CO₂

3. ER: 0.324 CS₂ LR: 0.0300 O₂

Identify the limiting and excess reactant when 75.78 g of Al reacts with 82.84 g of CuCl₂ to form AlCl₃ and Cu

Formula: 2Al + 2CuCl₂ → 2AlCl₃ + 2Cu

1. 82.84 × 1/134.45 × 3/3 = 0.6161

2. 75.78 × 1/26.98 × 3/2 = 4.213

3. ER: Al 4.213 LR: CuCl₂ 0.6161

Identify the limiting and excess reactant when 356.25 g of AgNO₃ reacts with 414.12 g of KCl to form KNO₃ and AgCl

Formula: KCl + AgNO₃ → KNO₃ + AgCl

1. 356.25 × 1/169.88 × 1/1 = 2.097

2. 414.12 × 1/74.55 × 1/1 = 5.555

3. ER: KCl 5.555, LR: AgNO₃ 2.097

Identify the limiting and excess reactant when 297.81 g of Pb(NO₃)₂ reacts with 125.24 g of K₂S to produce PbS and KNO₃. If 175 g of PbS is collected, what is the percent yield?

Formula: Pb(NO₃)₂ + K₂S → PbS + 2KNO₃

1. 297.81 × 1/331.22 × 1/1 × 239.26/1 = 215.11

2. 125.24 × 1/110.26 × 1/1 × 239.26/1 = 271.76

3. (175/215.11) * 100 = 81.35%

Moles of solute per liters of solution

Molarity

The substance being dissolved

A solute

A solution that contains the maximum amount of dissolved solute

Saturated solution

The maximum amount of a substance that can be dissolved in water at a specific temperature

Solubility

A solution with more dissolved solute than a saturated solution contains under the same conditions

Supersaturated solution

A solution that contains less solute than a saturated solution under the same conditions

Unsaturated solution

Describe the process of creating a saturated solution

You keep adding a solvent to a solute until no more solvent can dissolve and it begins to settle at the bottom of the solution

Describe how two solutions can have the same concentration while having different volumes

They can have the same ratio from solvent to solute

What are some factors that affect solubility?

Temperature, pressure, chemical nature of the solvent.

What are some factors that do NOT affect solubility?

The amount of solute, surface area, yeah I couldn’t find anymore but those 2 should be good enough

Describe the creation of 234 mL of a 3.2 M sodium chloride solution. (hint: calculate the number of grams you would need)

234 × 1/1000 × 3.2/1 × 58.44/1 = 43.76 grams

How many liters of a 3.2 M NaCl solution are required if 85 grams of sodium chloride are needed for a reaction?

1. 85 × 1/58.44 × 1/3.2 = 0.45

What is the concentration of a solution that has had 35 mL diluted to 500 mL with a new concentration of 0.45 M?

1. M₁V₁ = M₂V₂

2. We need M₁ so (0.45 × 500) / 35

3. 6.43

What is the molarity of a 654 mL of solution with 54 grams of calcium carbonate dissolved?

1. 54 g / 0.654 L * 1/100.09

2. 0.83

How many grams of strontium sulfate can be created from the reaction of 453 mL of a 3.4 M strontium chloride solution with an excess of 6.4 M ammonium sulfate solution? If the reaction as a 75% yield how many grams of strontium sulfate would be created in the lab?

1. Balance & create equation

2. SrCl₂ (aq) + (NH₄)₂SO₄ (aq) → SrSO₄ (s) + 2NH₄Cl(aq)

3. 0.453 × 3.4/1 × 1/1 × 183.68/1 = 282.90

4. 282.90 * .75 = 212.18

How many grams of potassium chloride can be dissolved in 543 grams of water at 55 degrees celsius?

543 × 45/100 = 244.35