Exam 1 Flashcards
(158 cards)
1
Q
What does alcohol chemicals always end in
A
-ol
2
Q
what is chem
A
matter and the changes it undergoes
3
Q
what is matter
A
has mass and takes up space
4
Q
nanoscale
A
atoms/molecules (h2o)
5
Q
macroscale
A
what we see in the living world (cup of water)
6
Q
physical properties
A
measurable or observable property that does not alter the identity of the material
7
Q
examples of physical properties
A
color, volume, freezing point, melting point, mass (weight),odor
8
Q
chemical properties
A
describes reactivity
-identity of materials will change
9
Q
examples of chemical properties
A
flammability, combustion
10
Q
Intensive properties
A
do not depend on amount of material present
-melting point, freezing point,boiling point, density,color
11
Q
extensive properties
A
depend on amount of material present
-mass, volume
12
Q
reaction formula
A
Left: reactants Right: product
h2o(s) –> h2o(l)
13
Q
physical change
A
occurs but does not alter identity
-water melting
14
Q
chemical change
A
alters identity, allows bonds to break and new atom combinations to form
-combustion
15
Q
what are signs of a chemical change
A
bubbles
color changes
new smells
new temperature
16
Q
solid
A
lots of interactions between close packed particles, order
definite shape
definite volume
17
Q
liquid
A
moderate interactions distance between particles varies
indefinite shape
defintie volume
18
Q
H
A
hydrogen
19
Q
He
A
helium
20
Q
Li
A
lithium
21
Q
Be
A
beryllium
22
Q
B
A
boron
23
Q
C
A
carbon
24
Q
N
A
nitrogen
25
O
oxygen
26
F
flourine
27
Ne
neon
28
Na
sodum
29
Mg
magnesium
30
al
aluminum
31
si
silicon
32
p
phosphorus
33
s
sulfer
34
cl
clorine
35
ar
argon
36
k
potassium
37
ca
calcium
38
sc
scandium
39
ti
titanium
40
v
vanadium
41
cr
chromium
42
mn
manganese
43
fe
iron
44
co
cobalt
45
ni
nickel
46
cu
copper
47
zn
zinc
48
ga
gallium
49
ge
germanium
50
as
arsenic
51
se
selenium
52
br
bromine
53
kr
krypton
54
gas
large separation between particles, no interaction between particles
- indefinite shape
- indefinite volume
- -only compressible state
55
two principle classes of matter
1. pure substance
| 2. mixture
56
two types of pure substances
1. element (1 type of atom)
| 2. compound (2+ types of atoms bonded)
57
two types of Mixtures
1. homogeneous - uniform throughout
| 2. heterogeneous - not uniform throughout
58
three physical processes to separate a mixture
1. object selection
2. filtration
3. distillation
59
element
only one the of atom involved, cannot be broken down into something simpler
60
monotomic
most elements - only one atom
61
diatomic
7 atoms, always found with two particles
62
what are the 7 diatomic atoms
```
I2 I
Br2 bring
Cl2 clay
F2 for
O2 our
N2 new
H2 home
```
63
Compound
chemical combination of 2+ elements
- atoms bonded together into a single unit
- makes a molecule
64
mixture
physical combination of 2+ pure substances
| -all pure substances in mixture retain their own chemical identity
65
homogeneous mixture
evenly distributed throughout
| -aka a solution
66
mixtures of gas are always....
homogeneous
67
heterogeneous mixture
top does not equal bottom
| yours does not equal mine
68
mass
kilogram
69
length
meter
70
time
second
71
temp
kelvin
72
amount of a substance
mole
73
giga
10^9
74
mega
10^6
75
kilo
10^3
76
deci
10^-1
77
centi
10^-2
78
milli
10^-3
79
micro
10^-6
80
nano
10^-9
81
Conversion factor
relates two units
| ie $1 = 4 quarters
82
dimensional analysis/stolchiometry
setting up math to allow for unit conversions
83
who proposed the atomic theory based on four postuates
John Dalton
84
Four postulates
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
what did daltons atomic theory explain
1. the law of constant composition
2. the law of conservation of mass
3. the law of multiple conversions
86
the law of multiple conversions
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
JJ Thompson
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
Millikan
oil drop
89
Isotope
Forms of an element with same number of protons but different number of neutrons
90
Atomic weight formula
Sum of all (isotope)(abundance as decimal)
91
H atomic weight
(1H mass)(abundance)+(2h mass)(abundance)+(3h mass)(abundance)
92
Molecules
A collection of non metal atoms
| All atoms must be found on right side of staircase and hydrogen
93
Covalent bond
Between atoms that share electrons
Can be single, double, or triple
Between a nonmetal & non metal
94
Naming of covalent bonds
```
Based on number of each specific atom in compound,
Must use prefix
Mono
Di
Tri
Tetra
Penta
```
95
Metal atoms in an ionic compound
Lose electrons
| -positive: cation
96
Non mental atoms in an ionic compound
Gain electrons
| -negative: anion
97
How to name ionic compound
Cation (metal), anion (non metal
98
How are ionic bonds connected
Stuck together by electrostatic attraction
99
Exceptions of ions
NH4+ polyatomic cation ammonium
| NH4Cl ionic
100
H+
hydrogen ion
101
Li+
litium ion
102
Na+
sodium ion
103
K+
potassium ion
104
Cs+
cesium ion
105
Ag+
silver ion
106
Mg2+
magnesium ion
107
Ca2+
calcium ion
108
Sr2+
strontium ion
109
Ba2+
barium ion
110
Zn2+
zinc ion
111
Cd2+
Cadmium ion
112
Al3+
aluminum ion
113
NH4+
ammonium ion
114
Cu+
copper(I) or Cuprous ion
115
Co2+
cobalt(II) or cobaltous ion
116
Cu2+
copper (II) or cupric ion
117
Fe2+
iron (II) or ferrous ion
118
Mn2+
Maganese(II) or manganous ion
119
Hg2^2+
mercury (I) or mercurous ion
120
Hg^2+
mercury(II) or mercuric ion
121
Ni2+
Nickel(II) or nickels ion
122
Pb2+
lead(II) or plumbous ion
123
Sn2+
Tin(II) or stannous ion
124
Cr3+
chromium(III) or chromatic ion
125
Fe3+
Iron(III) or ferric ion
126
H-
Hydride ion
127
F-
floride ion
128
Cl-
chloride ion
129
Br-
bromide ion
130
I-
iodide ion
131
Cn-
cynide ion
132
OH-
Hydroxide ion
133
O^2-
oxide ion
134
O2^2-
peroxide ion
135
S2-
Sulfide ion
136
N3-
Nitride ion
137
CH3COO- (or C2H3O2-)
Acetate ion
138
CIO3-
Chlorate ion
139
CLO4-
perchlorate ion
140
NO3-
Nitrate ion
141
MnO4-
permanganate ion
142
CO3^-2
carbonate ion
143
CrO4^-2
dichromate ion
144
SO4^-2
sulfate ion
145
PO4^-3
Phosphate ion
146
polyatomic ions
group of atoms covalently bonded together BUT has a charge
| -----NH4+
147
oxyanions w/o halogens
More molecules of O: -ate
| Less molecules of O: -ide
148
Oxyanions w/ halogen
4 per-__-ate
3 -ate
2 -ite
1 hypo-___-ite
149
How to balance reactions
coefficients
150
Aqueous solution
salt disolved in water
151
metal+non metal=
salt! which contains ions, so make ions first
152
Combustion reaction
Involved compounds hydrocarbons organic hydrocarbons (H,C,O)
| Burn in o2, burn in “air” only o2 involved
153
Hydrocarbon + o2
CO2(g)+H2O(g)+heat
154
Formula weight
Sum of atomic weights of atoms present in formula unit
| -ions (salts)
155
Molecular weight
Sum of atomic weights of atoms present in molecule
| -covalent bond (molecules)
156
At room temperature ionic bonds/salts are always
Solid crystal
157
Percent composition
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
1 mole/Avogadros number
Collection of 6.02x10^23 items
| -only ever items you can’t see
