Semester 2 Final

Question 1

Diatomics

Answer 1

H2 N2 O2 F2 Cl2 Br2 I2

Question 2

5 types of reactions

Answer 2

1. Synthesis (Composition or Combination)
2. Decomposition
3. Single Replacement
4. Double
5. Replacement
   Combustion

Question 3

Synthesis reaction

Answer 3

A + B = AB

Question 4

Decomposition reaction

Answer 4

AB = A + B

Question 5

Single replacement reaction

Answer 5

A + BC = AC + B

Question 6

Double replacement reaction

Answer 6

AB + CD = BC + AD
(Inner + Outer)

Question 7

Combustion reaction

Answer 7

Always produces CO2 & H20

Question 8

Law of conservation of mass

Answer 8

Each side of a chemical equation must have the same amount of atoms of each element

Question 9

Mole/Avogadro’s number

Answer 9

6.02 x 10^23

Question 10

Molar mass

Answer 10

g/mol or mol/g

Question 11

Atomic mass

Answer 11

Mass of an element on the periodic table Always has 2 decimals

Question 12

Particles for monoatomic elements

Answer 12

1 mol = Avogadro’s number atoms

Question 13

Particles for molecular compounds and diatomic elements

Answer 13

1 mol = Avogadro’s number molecules

Question 14

Particles for ionic compounds

Answer 14

1 mol = Avogadro’s number formula units

Question 15

Particle conversion

Answer 15

mol/Avogadro’s number particles

Avogadro’s number particles/mol

Question 16

2 step mole conversion

Answer 16

Mass in grams > Moles > Particles
And vice versa

Question 17

Percent composition

Answer 17

(Part/Whole) x 100

Question 18

Percent composition by mass

Answer 18

(mass of element/ mass of compound) x 100

Question 19

Percent composition by formulas

Answer 19

(molar mass of element/ molar mass of compound) x 100

Question 20

Empirical formula

Answer 20

Smallest whole number ratio of atoms in a compound
Divide elements/compounds when in grams by their molar mass to determine their subscript
When you are only given percents, assume the sample is 100.0g

Question 21

Hydrates

Answer 21

Compounds that are
chemically bonded to water molecules

Question 22

Naming hydrates

Answer 22

Use molecular compound prefixes for the moles of water and attach the name “hydrate”

Question 23

Molecular formula

Answer 23

“True Formula” - the actual number of atoms in a compound

Question 24

Calculating molecular formula

Answer 24

1. Find the empirical formula.
2. Find the empirical formula mass.
3. Divide the molecular mass by the empirical mass.
4. Multiply each subscript by the answer from step 3.

Question 25

Mole ratio

Answer 25

Coefficient ratio Moles wanted (coefficient)/Moles given (coefficient)

Question 26

Mole to mole conversion

Answer 26

Moles given x mole ratio

Question 27

Moles to mass conversion

Answer 27

Moles given x mole ratio x molar mass

Question 28

Mass to mass conversion

Answer 28

Mass given x molar mass x mole ratio x molar mass

Question 29

Percent yield

Answer 29

(Actual mass of product/ Theoretical mass of product) x 100

Question 30

Actual mass

Answer 30

Data from a real experiment or procedure

Question 31

Theoretical mass

Answer 31

Stoichiometry calculations

Question 32

Limiting reactant

Answer 32

Limits the amount of product that can be produced

Question 33

Excess reactant

Answer 33

Reactant that is left unused after a reaction

Question 34

Calculating limiting reactants

Answer 34

Put compounds through 3 step conversion into the product and see which produces less, this is your limiting reactant because it limits the amount of product that can be made

Question 35

Kinetic theory

Answer 35

1. Gas particles are small, hard spheres with insignificant volume 2. Gas particles are in rapid, constant, & random motion 3. All collisions between gas particles are perfectly elastic

Question 36

Absolute zero

Answer 36

0K

Question 37

Gas pressure

Answer 37

1atm=101.3kP=760mm Hg=760 torr

Question 38

Gas volume

Answer 38

1L=1dm³=100cm³=1000ml

Question 39

Gas at STP

Answer 39

273K and 1atm or 101.3kPa and 22.4 L/mol

Question 40

Boyle's law

Answer 40

P1 x V1 = P2 x V2

Question 41

Charles' law

Answer 41

V1/T1 = V2/T2

Question 42

Gay-Lussac' law

Answer 42

P1/T1 = P2/T2

Question 43

Combined gas law

Answer 43

P1V1/T1 = P2V2/T2

Question 44

Gas stoichiometry

Answer 44

Use Gas at STP and stoichiometry

Question 45

Dalton's law

Answer 45

Ptotal = P1 + P2 + P3 ...

Question 46

Ideal Gas law

Answer 46

PV = nRT

Question 47

Solute

Answer 47

Thing being dissolved

Question 48

Solvent

Answer 48

Dissolving medium

Question 49

Unsaturated solution

Answer 49

More solute dissolves

Question 50

Saturated solution

Answer 50

No more solute dissolves

Question 51

Supersaturated solution

Answer 51

Solute does not completely dissolve; not enough solvent to dissolve all of the solute

Question 52

Factors that affect solubility

Answer 52

1. Stirring 2. Temperature 3. Particle size

Question 53

Like dissolves like

Answer 53

Non-polar dissolves non-polar and Polar dissolves in water and other polar solvents

Question 54

Molarity

Answer 54

M = Moles of solute/L of solute

Question 55

Use molarity to prepare a solution

Answer 55

g = M x L x molar mass

Question 56

Dilution

Answer 56

M1V1 = M2V2

Question 57

Properties of acids

Answer 57

Turns litmus red H+ > OH-

Question 58

Properties of bases

Answer 58

Turns litmus blue OH- > H+

Question 59

Binary acids

Answer 59

2 elements Hydro prefix + Root + ic acid

Question 60

Ternary acids

Answer 60

More than 2 elements If it ends in -ate, turn to -ic acid If it ends in -ite, turn to -ous acid

Question 61

Bases

Answer 61

Simply add hydroxide

Question 62

Acid base neutralizing reaction

Answer 62

Always produces a form of salt and water

Question 63

Endothermic

Answer 63

Absorbes energy/heat

Question 64

Exothermic

Answer 64

Releases energy/heat

Question 65

Heat calculations

Answer 65

q = mc^T

Question 66

q

Answer 66

qhot + qcold = 0