Exam 1 (1-6) Flashcards
(144 cards)
1
Q
scientific notation
A
to the right is NEGATIVE
2
Q
scientific notation
A
to the left is POSITIVE
3
Q
multiply / divide sig figs
A
number with least number of sig figs
4
Q
add / subtract sig figs
A
number with least number of decimal points
5
Q
deci
A
-1
6
Q
centi
A
-2
7
Q
milli
A
-3
8
Q
micro
A
-6
9
Q
nano
A
-9
10
Q
pico
A
-12
11
Q
femto
A
-15
12
Q
kilo
A
3
13
Q
mega
A
6
14
Q
giga
A
10
15
Q
metric length unit
A
meter
16
Q
SI length unit
A
meter
17
Q
metric volume unit
A
Liter
18
Q
SI volume unit
A
cubic meter
19
Q
metric temperature unit
A
celsius
20
Q
SI temperature unit
A
K
21
Q
measured vs exact numbers
A
measured = obtained by measuring devices & are never exact
exact = counted our definitions in measurements with never ending # of sigs
22
Q
density =
A
mass / volume
23
Q
units for density
A
g / mL
24
Q
pure substances
A
elements
compounds
25
elements
1 element
26
compounds
2+ elements chemically bonded
27
mixtures
2+ compounds physically combined
homogeneous
heterogeneous
28
homogeneous
2+ compounds
same composition throughout
29
heterogeneous
2+ compounds
NO uniform composition
30
solids
definite shape
definite volume
31
liquids
NO definite shape
definite volume
32
gas
NO definite shape
NO definite volume
33
physical properties
change in physical state / shape
does NOT alter chemical composition or identity
34
chemical properties
ability of substance to interact with others and to change into another
change is in the composition or identity
35
energy
capacity to do work
36
kinetic energy
energy of motion
37
potential enegry
stored energy
38
thermal energy
energy released as heat
39
units of heat
calorie or joule
40
metric unit of heat
calorie
41
SI unit of heat
joule
42
conversion Cal to cal
1 Cal = 1,000 calories
43
conversion cal to joules
1 cal = 4.184 joules
44
what is the definition of a calorie
heat needed to raise the temperature by 1C of 1 g
45
C to K conversion
K = C +273
46
C to F conversion
F = 1.8C +32
47
equation for specific heat
q / (mass)(change in temp)
48
q in specific heat equation
heat transfered
metric = calories
SI = joules
49
mass in specific heat equation
grams
50
change in temperature in specific heat equation
Celsius
51
metals vs nonmetals
metals:
conductors
malleable / ductile
shiny
nonmetals:
not conductors
not malleable or ductile
brittle
52
metalloids
in between properties of metals and nonmetals
53
groups of periodic table
alkali metals
alkaline earth metals
transition elements
halogens
noble gases
54
what is the smallest unit of an element
an atom
55
protons
positive charge
inside nucleus
1 amu
56
who discovered proton
ruther ford
gold foil experiment
(atom is mostly empty space)
57
neutrons
neutral charge
inside nucleus
1 amu
58
who discovered neutron
chadwick
59
electrons
negative charge
in energy shells
1/2000 of an amu
60
who discovered electron
jj thompson
cathode ray
61
atomic number
number of protons and electrons
62
atomic mass
average weight of all isotopes
63
mass #
number of protons and neutrons
64
isotopes have same / different what
same P
different N
65
how to calculate atomic mass
(mass x abundance) + (mass x abundance)
for all isotopes
66
how many energy levels are there
7
67
higher energy level = ____ energy
higher
68
how many sublevels are there
4
s,p,d,f
69
how many orbitals does s have
1
70
how many orbitals does p have
3
71
how many orbitals does d have
5
72
how many orbitals does f have
7
73
how many electrons are in orbitals
2 in each orbital
74
what is an orbital
space where probability is high to find electrons
75
electron configuration
coefficient
letter
superscript
76
what does coefficient of electron configuration mean
energy level
77
what does letter of electron configuration mean
sublevel
78
what does superscript of electron configuration mean
number of electrons in the sublevel
79
valence electrons
electrons in outermost energy level
80
how to determine valence electrons
electron configuration
(count electrons in last energy level --- coefficient)
group number
81
electron dot symbol
lewis structure
indicates valence electrons as dots
82
atomic radii across a period
decreases
83
atomic radii down a group
increases
84
ionization energy across a period
increases
85
ionization energy down a group
decreases
86
metallic character across a period
decreases
87
metallic character down a group
increases
88
reason for atomic trends across a period
increase in protons increases the effective nuclear charge
89
reason for atomic trends down a group
increase in energy levels
90
zeff =
Z - S
total electrons - shielding electrons (nonvalence)
91
ionic compound
metal + nonmetal
loss / gain of electrons
92
covalent compound
nonmetal + nonmetal
sharing of electrons
93
cation
positive ion
loss of electrons
94
anion
negative ion
gain electrons
95
cations size
cations = smaller than atoms
more P compared to E means stronger pull on Es
96
anions size
anions = larger than atom
more electrons = weaker pull
97
name for ionic compounds
M + NM
metal = name
nonmetal = name end with "ide"
98
metals with variable change
most transition elements + Tin and Lead
99
name for metals with variable change
same as regular ionic compounds
add roman numeral to metal to clarify which ion it forms
100
polyatomic ions
2+ atoms with a charge
101
name for polyatomic ions
metal = name
ion = name ending with "ate"
102
ite
polyatomic ion with 1 less O
103
hydro - ous
polyatomic ion with 2 less O
104
per
polyatomic ion with 1 more O
105
hydrogen OR bi
polyatomic ion with 1 more H+
106
carbonate
CO3 -2
107
sulfate
SO4 -2
108
phosphate
PO4 3-
109
nitrate
NO3 -1
110
chlorate
ClO3 -1
111
fluroate
FO3 -1
112
iodate
IO3 -1
113
bromate
BrO3 -1
114
hydroxide
OH -1
115
ammonium
NH4 +1
116
name for covalent compounds
NM + NM
1st = name
2nd = name ending it "ide"
prefixes describe number of each (no charge)
117
prefixes for covalent compounds
mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca
118
states of ionic vs covalent
ionic = s at room temp
covalent = l / g at room temp
119
bonds in ionic compounds
ionic bonds
120
bonds in covalent compounds
intermolecular forces:
hydrogen
dipole-dipole
london dispersion forces
121
hydrogen bonds
POLAR
intermolecular forces between H & very electronegative atom
hydrogen + NOF
N, O, F
122
dipole-dipole forces
POLAR
second strongest
123
dispersion forces
NONPOLAR
weakest
124
vsepr steps
1.) lewis dot structure
2.) delta EN
3.) polarity, geometry, shape
125
geometry: 2 groups around central atom
linear
126
linear geometry:
2 groups bonded
1 group bonded
linear
linear
127
geometry: 3 groups around central atom
trigonal planar
128
trigonal planar geometry:
3 groups bonded
2 groups bonded
1 group bonded
trigonal planar
bent
linear
129
geometry: 4 groups around central atom
tetrahedral
130
tetrahedral geometry:
4 groups bonded
3 groups bonded
2 groups bonded
tetrahedral
trigonal pyramidal
bent
131
what is a "group" in vsepr
atom with bond
lone electron pair
(single, double, and triple bonds are all considered 1)
132
nonpolar electronegativity
0 - 0.4
133
polar electronegativity
0.5 - 1.8
134
ionic electronegativity
1.8 +
135
arrows in lewis structure go which way
arrows point towards more electronegative atom
represents a dipole
136
what is a dipole in lewis structure
arrow that points towards more electronegative atom
137
if bonds are nonpolar, molecule is ___
ALWAYS nonpolar
138
if bonds are polar, molecule is ___
polar OR nonpolar
if dipoles cancel out based on geometry, its NP, if not its polar
139
when do atoms become partially positive or negative
covalent bonds
the atom that keeps electrons most of the time becomes partially negative
others become partially positive
140
transition elements that do NOT have variable change
Silver (+1)
Zinc (+2)
Cadmium (+2)
141
Zinc ion charge
+2
142
Cadmium ion charge
+2
143
Silver ion charge
+1
143
Silver ion charge
+1
