1 semester test Flashcards
(90 cards)
1
Q
extensive property
A
changes with the amount
2
Q
intensive property
A
does not change with the amount
3
Q
6 signs of chemical change
A
- color change
- temperature change
- odor
- precipitate
- light emitted
- gas produced
4
Q
magic 7 diatomic elements
A
- H
- N
- O
- F
- Cl
- Br
- I
5
Q
liquid to gas
A
evaporation
6
Q
gas to solid
A
deposition
7
Q
solid to liquid
A
melting
8
Q
liquid to solid
A
freezing
9
Q
solid to gas
A
sublimation
10
Q
gas to liquid
A
condensation
11
Q
what is accuracy
A
correctness
12
Q
what is precision
A
reproducibility
13
Q
percent error formula
A
%error=(actual-measured)/actualx100
14
Q
1kg is how many grams
A
1000
15
Q
1km is how many m
A
1000
16
Q
100 cm is how many m
A
1
17
Q
1000mm is how many m
A
1
18
Q
1000mL is how many L
A
1
19
Q
Dalton’s theory
A
- all matter is composed of tiny indivisible particles called atoms (true)
- all atoms of an element are identical (false)
- atoms cannot be created, divided, or destroyed (false, atoms can be divided)
- atoms of different elements combine chemically to form compounds(true)
- atoms of 1 element cannot change into a new element during chemical reactions (true)
20
Q
who experimented with the cathode ray tube
A
JJ Thompson
21
Q
who used the gold foil experiement
A
Ernest Rutherford
22
Q
who discovered the existence of neutrons
A
James Chadwick (jimmy neutron)
23
Q
who proposed that electrons are arranged in 7 circular orbits
A
Niels Bohr
24
Q
isotope notation
A
potassium-39 or 39
K
19
25
average atomic mass formula
(%abundance X mass #) + (%abundance X mass#)
26
how do cations form positive ions
lose electrons
27
how do anions form negative ions
gain electrons
28
what is an atom
single element
29
what is a molecule
compound of two or more non metals
30
what is a formula unit
compound with a metal bonded to non metal
31
how many electrons can an orbital hold
2 electrons
32
what is the ground state
most stable, lowest energy arrangement of the electrons in an atom
33
what is the excited state
atom gains energy and electrons jump into higher energy levels
34
ground to excited
absorb energy
35
excited to ground
release energy
36
representative element for atomic radii or ionic radii
Fr Francium
37
representative element ionization energy
He Helium
38
representative element for electronegativity
F Fluorine
39
what is a metallic bond
2 or more metals
40
physical properties of metallic bonds
electrons are mobile = conduct electricity & heat
atoms are hard to pull apart bc of sea of e-
ductile and malleable
41
ionic bonding
bonding between 2 ions (nm and m)
42
what is the polyatomic symbol and charge for acetate
C2H3O2 -1
43
what is the polyatomic symbol and charge for nitrite
NO2 -1
44
what is the polyatomic symbol and charge for nitrate
NO3 -1
45
what is the polyatomic symbol and charge for hydroxide
OH -1
46
what is the polyatomic symbol and charge for carbonate
CO3 -2
47
what is the polyatomic symbol and charge for sulfite
SO3 -2
48
what is the polyatomic symbol and charge for sulfate
SO4 -2
49
what is the polyatomic symbol and charge for phosphite
PO3 -3
50
what is the polyatomic symbol and charge for phosphate
PO4 -3
51
what is the polyatomic symbol and charge for ammonium
NH4 +1
52
what is the polyatomic symbol and charge for hydronium
H3O +1
53
covalent bonds are the result of the sharing of what
valence electrons
54
linear molecular shapes have what bond angles
180
55
trigonal planar molecular shapes have what bond angles
120
56
tetrahedral molecular shapes have what bond angles
109.5
57
trigonal pyramidal molecular shapes have what bond angles
107.3
58
bent molecular shapes have what bond angles
104.5
59
what is an alloy
mixture of 2 or more metals
60
what is the strongest bond
ionic
61
what bond has the highest melting point
ionic
62
what bond has the lowest melting point
covalent
63
what is the weakest bond
covalent
64
what is the strongest bond
ionic
65
mono
1
66
di
2
67
tri
3
68
tetra
4
69
penta
5
70
hexa
6
71
hepta
7
72
octa
8
73
nona
9
74
deca
10
75
nitrogen trihydride NH3 is what
ammonia
76
carbon tetrahydride CH4 is what
methane
77
no "O" means to
use prefix "hydro" Hydro___ic acid
78
with "O" means to
not use "hydro"
79
ate to
ic
80
ite to
ous
81
moles flow chart
grams moles particles (funs to ions, atoms, molecules to atoms)
82
what is empirical formula
simplest whole # (reduced)
83
what is molecular formula
the real formula (not reduced)
84
4 steps to writing empirical formula
1. determine number of grams for each element (% to g)
2. turn grams into moles for each element
3. divide by smallest mole # (keep 4 decimals)
4. if not all whole numbers, multiply to get whole #
85
molecular formula
molecular mass of compound/empirical mass of compound (real/reduced)
86
In the formula C=λν, what is the value of the C constant
speed of light 3x10^8
87
in the formula E=hν, what is the value of the h constant
planck's constant 6.63x10^-34
88
for polarity, 0.3 and below is
non polar
89
for polarity, 0.3 to 1.7 is
covalent
90
for polarity, 1.7 and above is
ionic
