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Chem 1610 > Midterm 1 (Chapters 1-4) > Flashcards

Midterm 1 (Chapters 1-4) Flashcards

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1
Q

Metric System

A 
Peta 15
Tera 12
Giga 9
Mega 6
Kilo 3
Deci -1 
Centi -2
Milli -3
Micro (u) -6
Nano -9
Pico -12
Femto -15
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2
Q

Cathode Rays

A
  • electrons move from cathode (-) to anode (+)
  • rays are deflected by magnet
  • no air in the tube
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3
Q

Millikan Oil Experiment

A
  • found the charge of an electron: 1.602 x 10^-19

- used x rays to charge drops of oil between two plates, one positive and one negative

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4
Q

charge of an electron

A

1.602 x 10^-19 C

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5
Q

radiation

A

alpha: protons
beta: electrons
gamma: neutral

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6
Q

ammonium

A

NH4+

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7
Q

aluminum ion

A

Al+3

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8
Q

oxyanions

A

per ate (ClO4- perchlorate)
at (ClO3- chlorate)
ite (ClO2- chlorite)
hypo ite (ClO hypochlorite)

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9
Q

nitrate

A

NO3-

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10
Q

nitrite

A

NO2-

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11
Q

sulfate

A

SO4-2

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12
Q

phosphate

A

PO4-3

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13
Q

nitride

A

N-3

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14
Q

oxyanions –> acid

A

ate –> ic
ite –> ous

ClO4: perchlorate –> HClO4 perchloric acid
ClO3: chlorate –> HClO3 chloric acid
ClO2: chlorite –> HClO2 chlorous acid
ClO: hypochlorite –> HClO hypochlorous acid

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15
Q

sulfite

A

SO3-2

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16
Q

7 strong acids

A

HBr, HI, HCl, HClO4, HClO3, H2SO4, HNO3

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17
Q

8 strong bases

A 
group 1 and heavy 2's
LiOH
NaOH
KOH
RbOH
CsOH
CaOH
SrOH
BaOH
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18
Q

is NH4 weak or strong?

A

ionic compounds containing NH4+ are weak

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19
Q

ionized vs. dissociated

A

molecular compounds ionize in water and ionic compounds dissociate in water

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20
Q

which anions are always soluble?

A

NO3- and CH3COO- and NH4+

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21
Q

acetic acid

A

CH3COOH

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22
Q

Cl- solubility rules

A

always soluble except compounds of Ag+, Hg2+2, Pb+2

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23
Q

Br- solubility rules

A

always soluble except compounds of Ag+, Hg2+2, Pb+2

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24
Q

I- solubility rules

A

always soluble except compounds of Ag+, Hg2+2, Pb+2

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25
Q

SO4-2 solubility rules

A

always soluble except compounds of Sr+2, Ba+2, Hg2+2, Pb+2

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26
Q

S-2 solubility rules

A

insoluble except compounds of NH4+, alkali metals, Ca+2, Sr+2, Ba+2

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27
Q

CO3-2 solubility rules

A

insoluble except compounds of NH4+ and alkali metals

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28
Q

PO4-3 solubility rules

A

insoluble except compounds of NH4+ and alkali metals

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29
Q

OH- solubility rules

A

insoluble except compounds of NH4+, alkali metals, Ca+2, Sr+2, and Ba+2

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30
Q

ammonia

A

NH3: common base, weak base, weak electrolyte

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31
Q

strong electrolytes?

A

all ionic compounds and strong acids/bases are strong electrolytes

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32
Q

weak electrolytes?

A

all weak acids/bases, water, NH3

33
Q

nonelectrolytes?

A

all other compounds, usually molecular compounds like sugars, alcohols

34
Q

reaction of CO3-2 or HCO3-2 with an acid?

A

first gives carbonic acid (H2CO3) which then breaks down into H20 and cO2

35
Q

what combine with acids to form gases?

A

carbonates CO3 form CO2
sulfites SO3 form SO2
sulfides S form H2S

36
Q

what are the driving forces of chemical reactions?

A

1) precipitation formation
2) neutralization - formation of weak electrolyte (H20)
3) formation of a gas

37
Q

oxidation of hydrogen?

A

+1 when with nonmetals

-1 when with metals

38
Q

chromium oxidation states

A

Cr+3 is green

Cr+6 is orange

39
Q

activity series

A
  • elements at the top are most easily oxidized and react readily
  • metals on the list can be oxidized by the ions of the elements below it
40
Q

what is a pure substance?

A

matter that has distinct properties and a composition that does not vary from sample to sample: water/NaCl

41
Q

the observation that the elemental composition of a compound is always the same is known as…..

A

the law of constant compositions

42
Q

what are some physical properties?

A

color, odor, density, MP, BP, hardness, conductivity

43
Q

what are some chemical properties?

A

flammability, bubbles, heat, ppt, light

44
Q

intensive vs. extensive

A

intensive does not depends on the amount of sample: temperature, MP, BP

extensive properties: depend on amount of sample: mass/volume

45
Q

Kelvin to Celcius conversion

A

K = C + 273.15

46
Q

1 mL = 1 cm^3

A

conversion factor

47
Q

exact vs. inexact

A

s obtained by measurement are always inexact

48
Q

precision vs. accuracy

A

precise: you get the same answer multiple times
accurate: you get the right answer

49
Q

hypothesis

A

a possible explanation for certain phenomena based on preliminary experimental data

50
Q

theory

A

more general, has a significant body of experimental evidence to support it, an explanation of natural behavior, explains why matter behaves the way it does

51
Q

scientific law

A

summary or statement of natural behavior, tells how matter behaves

52
Q

determinate errors

A

the source can be identified and theoretically eliminated : e.g. you read the top of the meniscus instead of the bottom

53
Q

indeterminate error

A

cannot be identified: e.g. estimating the last digit

54
Q

density

A

g/mL or g/cm^3usually

55
Q

John Dalton’s Atomic Theory

A

1) each element is composed of extremely small particles called atoms
2) all toms of a given element are identical but the atoms of one element differ from the atoms of all other elements (false because of isotopes)
4) compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atom

56
Q

in a given compound, the relative numbers and kinds of atoms are constant

A

law of constant compositions - ratios are the same - this is pertaining to 1 molecule - no matter how much of the sample there is, the ratio will be the same H2O has 2 hydrogens and 1 oxygen no matter what

57
Q

the total mass of materials present after a chemical reaction is the same as the total mass present before the reaction - atoms are neither created nor destroyed

A

law of conservation of mass

58
Q

when two elements A and B form two different compounds, the masses of element B that combine with a fixed mass of element A can be expressed as a ratio of small whole numbers

A

law of multiple proportions: CO vs CO2

AB, AB2, AB3

if all masses of A are 1 g, then the mass of B in compound 1 vs. 2 vs. 3 are ratios X,Y,Z, and they’ll be ratios that are small whole numbers

C + O –> CO(AB) and CO2(AB2)
C is 1.0 g then O must be 1.33 g in CO and 2.67 g in CO2
2.67g/1.33g = 2

59
Q

J.J. Thomson

A

charge:mass ratio 1.76 x 10^8 coulombs/g

60
Q

angstrom to meters

A

1 A = 1 x 10^-10 m

61
Q

mass number

A

superscript number: protons + neutrons

62
Q

isotopes

A

same number of protons but different number of neutrons

63
Q

atomic number

A

number of protons - all atoms of the same element have the same number of protons - # e- = protons in a neutral atom

64
Q

average atomic weight

A

isotopes mass x fractional isotope abundance

65
Q

groups

A

vertical columns - usually have similar physical and chemical properties

66
Q

naming ionic and molecular compounds

A

ionic: metal and nonmetal: calcium chloride - name cation then anion
molecular: nonmetal and nonmetal: diphosphorous pentoxide - use prefixes

67
Q

anions derived by adding H+ to an oxyanion are named by adding….

A

hydrogen or bi as a prefix

CO3-2 carbonate ion –> H2CO3 hydrogen carbonate/bicarbonate ion

68
Q

deflection of particles between charged plates

A

if the particle is only slightly deflected then it has a large mass because heavier molecules are harder to move and linear momentum increases

69
Q

what happens when metal carbonates decompose?

A

metal carbonates decompose to form metal oxides and carbon dioxide

70
Q

what happens when metal chlorates decompose?

A

metal chlorates decompose to form metal chlorides and O2

71
Q

what happens when hydrocarbons combust?

A

hydrocarbons combust in air to form CO2 and H20

72
Q

molar mass

A

grams/mol

73
Q

MM to formula weight

A

MM in grams is equivalent to formula weight in amu

74
Q

empirical vs. molecular

A

empirical formula is the smallest whole number ratio combination - to get the molecular formula: molecular weight/ empirical formula weight to get a whole # multiple

75
Q

combustion analysis

A

you get a certain amount of CO2 and H20 and you find H and C from it and possibly another compound

76
Q

limiting reactant

A

USE ICE CHARTS

77
Q

percent yield

A

actual/theoretical (actual is the amount of product actually obtained, usually given to you)

78
Q

avogadro’s number

A

6.022x10^23 atoms

79
Q

molarity

A

moles of solute/liters of solvent

Chem 1610 (7 decks)

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