Exam 1

Question 0

Hydrate

Answer 0

A compound associated with a specific amount of water. Ex: FeCl3•6H2O

Question 1

Law of constant composition

Answer 1

The relative number/types of elements in a given substance, is equally distributed in every part of that sample.

Question 3

Atom

Answer 3

Smallest particle of an element that retains the chemical properties of that element. Ex: 8p+8n+10e- –> one oxygen atom

Question 4

Diatomic elements:

Answer 4

H2, N2, O2, F2, Cl2, Br2, I2 and Hg2 (when it has a -1 charge)

Question 5

SI Unit for length:

Answer 5

Meters: m

Question 6

SI Units for volume:

Answer 6

Liters: L

Derived from: 1cm^3+1cm^3+1cm^3= 1 mL

Question 7

Molecule

Answer 7

A set of two or more atoms joined together. Ex: h2, HCl, NO3
Diatomic: 2
Polyatomic: 3+

Question 8

SI Units for mass

Answer 8

Kilograms: kg

Question 9

SI Unit for time

Answer 9

Seconds: s

Question 10

Density formula

Answer 10

Density= mass/volume

D=m/v

Question 11

Mole:

Answer 11

A quantity equal to the number of atoms in exactly 12 grams of Carbon-12

Question 12

SI Unit for temperature

Answer 12

Kelvins: K

Question 13

Avogadro’s Number:

Answer 13

Number of atoms (particles, molecules, etc) in one mole of a substance: 6.022E23

Question 15

Calculating molecular mass/ formula mass

Answer 15

Add up the masses of each element, and multiply individual masses by the # present in the compound. Measured in amu’s

Question 16

Calculating molar mass

Answer 16

Add up molar masses of elements in the compound, then multiply by the same number as present

Question 17

Conversion between grams to moles

Answer 17

Divide by the molar mass (g/mol) of the substance

Question 18

Conversion from moles to number of atoms

Answer 18

Multiply moles by 6.022E23 (atoms/mole)

Question 19

Determining percent composition

Answer 19

(Assume 100g sample if not given) Take the total mass of the element and divide it by the total mass of the sample.

Question 20

Empirical formula:

Answer 20

Relative number of elements in the smallest possible ratio

Question 21

Calculating empirical formula:

Given elements and % comp

Answer 21

Assume a 100g sample with %comps. Calculate molar mass. Convert grams to moles. Divide all by the smallest number of moles calculated. Round to nearest whole #- that’s the # in the formula.

Question 22

Molecular formula:

Answer 22

Represents the relative number of elements according to the actual # of atoms. (True formula)

Question 24

Limiting reactant

Answer 24

The reactant(s) that are used up first in a reaction. Other reactants may have excess substance.

Question 25

Theoretical yield

Answer 25

Take amount of limiting reactant, convert it to mols. Convert mols of reactant to mols of product. Convert mols back to grams.

Question 26

Systematic error:

Answer 26

Consistent. Attributed to a device or procedure. Precise results, but inaccurate.

Question 27

Random error:

Answer 27

Inconsistent. Could be anything such as human error. Not precise nor accurate.

Question 28

Percent yield:

Answer 28

After actual yield is measured: divide (experimental mass yield by theoretical mass yield) then, multiply by 100.

Question 29

Intensive property:

Answer 29

Property that does not rely on the sample size. Examples: Boiling point, density, color, etc

Question 30

Extensive properties:

Answer 30

Properties that rely on sample size. Examples include volume, pressure, calories, etc)

Question 31

Stoichiometry:

Answer 31

The study of mass relations in chemical reactions. The conversion of mols of substance A to mols of another substance, B.

Question 32

Element types:

Answer 32

Metals Nonmetals Semi-metals (metalloids) Allotropes

Question 33

Electron

Answer 33

Negatively charged (-1) particle, relatively massless (almost 0 amu's at 5.485E-4)

Question 34

Proton:

Answer 34

A positively charged (+1) particle that has a mass of just over 1 amu at 1.007276

Question 35

Neutron:

Answer 35

A neutral particle with a relative mass of 1 amu

Question 36

Reliability of thesis's:

Answer 36

Hypothesis

Question 37

Peroxide:

Answer 37

O2 (2-)

Question 38

Superoxide:

Answer 38

O2 (1-)

Question 39

chromate:

Answer 39

CrO4 (2-)

Question 40

Dichromate:

Answer 40

Cr2O7 (2-)

Question 41

Permanganate:

Answer 41

MnO4 (1-)

Question 42

Carbonate:

Answer 42

CO3 (2-)

Question 43

Acetate:

Answer 43

C2H3O2 (1-)

Question 44

Bicarbonate/ | Hydrogen carbonate:

Answer 44

HCO3 (1-)

Question 45

Bisulfate/ | Hydrogen sulfate:

Answer 45

HSO4 (1-)

Question 46

Cyanide:

Answer 46

CN (1-)

Question 47

Ammonia:

Answer 47

HN3

Question 48

Signs of a reaction:

Answer 48

``` effervescence(bubbling, gas release) Luminescence (light) Color change Flame Precipitation(formation of solid) ```

Question 49

Ammonium:

Answer 49

NH4 (1+)

Question 50

Calculating Molecular Formula: | Given empirical and sample molar mass

Answer 50

Calculate molar mass of empirical equation. Divide given molar mass by emperical molar mass. Multiply answer by subscripts to reveal molecular formula.

Question 52

Naming oxyanions:

Answer 52

+1 O = (hy)per- - 1 O = -ite - 2 O = hypo- -ite Charge stays the same

Question 54

Phosphate:

Answer 54

PO4 (3-)

Question 55

Monoatomic anion naming:

Answer 55

Drop suffix, add -ide. | Examples: N (3-): nitride, Br(1-): Bromide, etc.

Question 56

Naming binary molecular compounds:

Answer 56

First element as it is, | Second element: add prefix equivalent to # of atoms present and with anion name (usually the suffix -ide)

Question 57

4 Main Branches of Chemistry:

Answer 57

``` Analytical (how much, ##) Physical (how, why) Inorganic(no C)(except CO,CO2) Organic (contains Carbon) (Others: biochem, nuclear) ```

Question 58

Sulfate:

Answer 58

SO4 (2-)

Question 59

Chlorate:

Answer 59

ClO3 (1-)

Question 60

Nitrate:

Answer 60

NO3 (1-)