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Chemistry 101 > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

What does alcohol chemicals always end in

A

-ol

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2
Q

what is chem

A

matter and the changes it undergoes

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3
Q

what is matter

A

has mass and takes up space

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4
Q

nanoscale

A

atoms/molecules (h2o)

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5
Q

macroscale

A

what we see in the living world (cup of water)

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6
Q

physical properties

A

measurable or observable property that does not alter the identity of the material

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7
Q

examples of physical properties

A

color, volume, freezing point, melting point, mass (weight),odor

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8
Q

chemical properties

A

describes reactivity

-identity of materials will change

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9
Q

examples of chemical properties

A

flammability, combustion

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10
Q

Intensive properties

A

do not depend on amount of material present

-melting point, freezing point,boiling point, density,color

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11
Q

extensive properties

A

depend on amount of material present

-mass, volume

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12
Q

reaction formula

A

Left: reactants Right: product

h2o(s) –> h2o(l)

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13
Q

physical change

A

occurs but does not alter identity

-water melting

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14
Q

chemical change

A

alters identity, allows bonds to break and new atom combinations to form
-combustion

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15
Q

what are signs of a chemical change

A

bubbles
color changes
new smells
new temperature

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16
Q

solid

A

lots of interactions between close packed particles, order
definite shape
definite volume

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17
Q

liquid

A

moderate interactions distance between particles varies
indefinite shape
defintie volume

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18
Q

H

A

hydrogen

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19
Q

He

A

helium

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20
Q

Li

A

lithium

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21
Q

Be

A

beryllium

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22
Q

B

A

boron

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23
Q

C

A

carbon

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24
Q

N

A

nitrogen

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25
Q

O

A

oxygen

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26
Q

F

A

flourine

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27
Q

Ne

A

neon

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28
Q

Na

A

sodum

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29
Q

Mg

A

magnesium

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30
Q

al

A

aluminum

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31
Q

si

A

silicon

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32
Q

p

A

phosphorus

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33
Q

s

A

sulfer

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34
Q

cl

A

clorine

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35
Q

ar

A

argon

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36
Q

k

A

potassium

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37
Q

ca

A

calcium

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38
Q

sc

A

scandium

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39
Q

ti

A

titanium

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40
Q

v

A

vanadium

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41
Q

cr

A

chromium

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42
Q

mn

A

manganese

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43
Q

fe

A

iron

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44
Q

co

A

cobalt

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45
Q

ni

A

nickel

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46
Q

cu

A

copper

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47
Q

zn

A

zinc

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48
Q

ga

A

gallium

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49
Q

ge

A

germanium

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50
Q

as

A

arsenic

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51
Q

se

A

selenium

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52
Q

br

A

bromine

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53
Q

kr

A

krypton

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54
Q

gas

A

large separation between particles, no interaction between particles

  • indefinite shape
  • indefinite volume
  • -only compressible state
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55
Q

two principle classes of matter

A
  1. pure substance

2. mixture

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56
Q

two types of pure substances

A
  1. element (1 type of atom)

2. compound (2+ types of atoms bonded)

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57
Q

two types of Mixtures

A
  1. homogeneous - uniform throughout

2. heterogeneous - not uniform throughout

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58
Q

three physical processes to separate a mixture

A
  1. object selection
  2. filtration
  3. distillation
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59
Q

element

A

only one the of atom involved, cannot be broken down into something simpler

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60
Q

monotomic

A

most elements - only one atom

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61
Q

diatomic

A

7 atoms, always found with two particles

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62
Q

what are the 7 diatomic atoms

A 
I2 I
Br2 bring
Cl2 clay
F2 for
O2 our
N2 new
H2 home
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63
Q

Compound

A

chemical combination of 2+ elements

  • atoms bonded together into a single unit
  • makes a molecule
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64
Q

mixture

A

physical combination of 2+ pure substances

-all pure substances in mixture retain their own chemical identity

65
Q

homogeneous mixture

A

evenly distributed throughout

-aka a solution

66
Q

mixtures of gas are always….

A

homogeneous

67
Q

heterogeneous mixture

A

top does not equal bottom

yours does not equal mine

68
Q

mass

A

kilogram

69
Q

length

A

meter

70
Q

time

A

second

71
Q

temp

A

kelvin

72
Q

amount of a substance

A

mole

73
Q

giga

A

10^9

74
Q

mega

A

10^6

75
Q

kilo

A

10^3

76
Q

deci

A

10^-1

77
Q

centi

A

10^-2

78
Q

milli

A

10^-3

79
Q

micro

A

10^-6

80
Q

nano

A

10^-9

81
Q

Conversion factor

A

relates two units

ie $1 = 4 quarters

82
Q

dimensional analysis/stolchiometry

A

setting up math to allow for unit conversions

83
Q

who proposed the atomic theory based on four postuates

A

John Dalton

84
Q

Four postulates

A
  1. each element is composed of extremely small particles called atoms
    - each element has it’s own kind of atom
  2. all atoms of a given element are identical in mass and properties
    - physical and chemical
  3. atoms are neither created nor destroyed during chemical reactions, and atoms of one element cannot be changed into atoms of another element
  4. atoms from different elements can combine to form compounds
    - oxygen+nitrogen=nitrogen monoxide (forms molecule)
85
Q

what did daltons atomic theory explain

A
  1. the law of constant composition
  2. the law of conservation of mass
  3. the law of multiple conversions
86
Q

the law of multiple conversions

A

if two elements combine to form more than one product the atoms will combine in whole number ratios

  • compounds possible when carbon combines w oxygen CO and CO2
  • -12g C + 16g O = CO
  • -12g C + 32 g O = CO2
87
Q

JJ Thompson

A

cathode ray tube

  • beam of light goes from cathode (-) to anode (+) and when (+) magnet is put behind it light attracts, when (-) magnet is put behind it light deflects
  • -beam is a beam of eelectrons
88
Q

Millikan

A

oil drop

89
Q

Isotope

A

Forms of an element with same number of protons but different number of neutrons

90
Q

Atomic weight formula

A

Sum of all (isotope)(abundance as decimal)

91
Q

H atomic weight

A

(1H mass)(abundance)+(2h mass)(abundance)+(3h mass)(abundance)

92
Q

Molecules

A

A collection of non metal atoms

All atoms must be found on right side of staircase and hydrogen

93
Q

Covalent bond

A

Between atoms that share electrons
Can be single, double, or triple
Between a nonmetal & non metal

94
Q

Naming of covalent bonds

A 
Based on number of each specific atom in compound, 
Must  use prefix
Mono
Di 
Tri 
Tetra 
Penta
95
Q

Metal atoms in an ionic compound

A

Lose electrons

-positive: cation

96
Q

Non mental atoms in an ionic compound

A

Gain electrons

-negative: anion

97
Q

How to name ionic compound

A

Cation (metal), anion (non metal

98
Q

How are ionic bonds connected

A

Stuck together by electrostatic attraction

99
Q

Exceptions of ions

A

NH4+ polyatomic cation ammonium

NH4Cl ionic

100
Q

H+

A

hydrogen ion

101
Q

Li+

A

litium ion

102
Q

Na+

A

sodium ion

103
Q

K+

A

potassium ion

104
Q

Cs+

A

cesium ion

105
Q

Ag+

A

silver ion

106
Q

Mg2+

A

magnesium ion

107
Q

Ca2+

A

calcium ion

108
Q

Sr2+

A

strontium ion

109
Q

Ba2+

A

barium ion

110
Q

Zn2+

A

zinc ion

111
Q

Cd2+

A

Cadmium ion

112
Q

Al3+

A

aluminum ion

113
Q

NH4+

A

ammonium ion

114
Q

Cu+

A

copper(I) or Cuprous ion

115
Q

Co2+

A

cobalt(II) or cobaltous ion

116
Q

Cu2+

A

copper (II) or cupric ion

117
Q

Fe2+

A

iron (II) or ferrous ion

118
Q

Mn2+

A

Maganese(II) or manganous ion

119
Q

Hg2^2+

A

mercury (I) or mercurous ion

120
Q

Hg^2+

A

mercury(II) or mercuric ion

121
Q

Ni2+

A

Nickel(II) or nickels ion

122
Q

Pb2+

A

lead(II) or plumbous ion

123
Q

Sn2+

A

Tin(II) or stannous ion

124
Q

Cr3+

A

chromium(III) or chromatic ion

125
Q

Fe3+

A

Iron(III) or ferric ion

126
Q

H-

A

Hydride ion

127
Q

F-

A

floride ion

128
Q

Cl-

A

chloride ion

129
Q

Br-

A

bromide ion

130
Q

I-

A

iodide ion

131
Q

Cn-

A

cynide ion

132
Q

OH-

A

Hydroxide ion

133
Q

O^2-

A

oxide ion

134
Q

O2^2-

A

peroxide ion

135
Q

S2-

A

Sulfide ion

136
Q

N3-

A

Nitride ion

137
Q

CH3COO- (or C2H3O2-)

A

Acetate ion

138
Q

CIO3-

A

Chlorate ion

139
Q

CLO4-

A

perchlorate ion

140
Q

NO3-

A

Nitrate ion

141
Q

MnO4-

A

permanganate ion

142
Q

CO3^-2

A

carbonate ion

143
Q

CrO4^-2

A

dichromate ion

144
Q

SO4^-2

A

sulfate ion

145
Q

PO4^-3

A

Phosphate ion

146
Q

polyatomic ions

A

group of atoms covalently bonded together BUT has a charge

—–NH4+

147
Q

oxyanions w/o halogens

A

More molecules of O: -ate

Less molecules of O: -ide

148
Q

Oxyanions w/ halogen

A

4 per-__-ate
3 -ate
2 -ite
1 hypo-___-ite

149
Q

How to balance reactions

A

coefficients

150
Q

Aqueous solution

A

salt disolved in water

151
Q

metal+non metal=

A

salt! which contains ions, so make ions first

152
Q

Combustion reaction

A

Involved compounds hydrocarbons organic hydrocarbons (H,C,O)

Burn in o2, burn in “air” only o2 involved

153
Q

Hydrocarbon + o2

A

CO2(g)+H2O(g)+heat

154
Q

Formula weight

A

Sum of atomic weights of atoms present in formula unit

-ions (salts)

155
Q

Molecular weight

A

Sum of atomic weights of atoms present in molecule

-covalent bond (molecules)

156
Q

At room temperature ionic bonds/salts are always

A

Solid crystal

157
Q

Percent composition

A

Tells you what portion of the entire mass of a substance is due to a specific type of atom
Atom amu/total amu x100%

158
Q

1 mole/Avogadros number

A

Collection of 6.02x10^23 items

-only ever items you can’t see

Chemistry 101 (4 decks)

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