Chapter 13 and 14 Flashcards
(107 cards)
1
Q
organized study of the composition and interaction of matter
A
chemistry
2
Q
substances composed of a single type of atom
A
element
3
Q
all matter consist of tiny particles called
A
atoms
4
Q
atoms of different elements can combine in specific ways to make compounds
A
true
5
Q
chemical processes are the result of the rearrangement combo or separation of atoms
A
true
6
Q
daltons atomic theory
A
7
Q
all atoms are made up of subatomic particles called electrons, neutrons, and protons according to dalton’s atomic theory
A
it is a true statement, but NOT according to Dalton’s atomic theory
8
Q
what are substances composed of atoms of 2+ elements bonded together
A
compounds
9
Q
aluminum symbol
A
Al
10
Q
barium symbol
A
Ba
11
Q
calcium symbol
A
Ca
12
Q
copper symbol
A
Cu
13
Q
Au
A
gold
14
Q
H
A
hydrogen
15
Q
He
A
helium
16
Q
Lead symbol
A
Pb
17
Q
magnesium symbol
A
Mg
18
Q
mercury symbol
A
Hg
19
Q
unique characteristic of mercury
A
liquid at room temperature
20
Q
Ne
A
neon
21
Q
Ni
A
nickel
22
Q
radon symbol
A
Rn
22
Q
tungsten symbol
A
W
23
Q
silver symbol
A
Ag
24
zinc symbol
Zn
25
U
uranium
26
protons neutrons and electrons belong to particles smaller than the atom called
subatomic particles
27
which 2 subatomic particles are nucleons
protons and neutrons
28
which subatomic particle has no charge
neutron
29
substance of the same element that differs in its mass number
isotope
30
supposed smaller particles making up protons and neutrons
quarks
31
what in an atom is composed of the protons and neutrons
nucleus
32
atom that gains or loses electrons
ion
33
mathematical equation used to determine the max amount of electrons that can reside in an energy level
(2n)(2n)
34
total number of protons and neutrons in an atom
mass number
35
if an isotope of carbon 14, and carbon has 6 protons, how many neutrons does that carbon atom have
8
36
which model of the atom first proposed that electrons resided in energy lvls around the nuecleus and is the most familiar model
bohr model
37
principle stating you can't know the position and the velocity of an electron simultaneously
Heisenberg uncertainty principle
38
every electron in an atom can be mathematically represented by 4 ______ numbers
quantum
39
which principle states that no 2 electrons can have the same 4 quantum numbers in an atom
pauli exclusion principle
40
which type of radioactive decay is the ejection of a electron from the nucleus
beta decay
41
ejection of 2 protons and 2 neutrons in radioactive decay
alpha decay
42
which type of decay can be stopped by a sheet of paper
alpha decay
43
which type of decay is the ejection of energy
gamma decay
44
what is the splitting apart of larger atoms into smaller atoms
fission
45
device initiating an uncontrolled chain reaction of atomic material
atomic bomb
46
a chain reaction can't occur unless their is a certain amount of fissionable mass present. It is called _______
critical mass
47
a device that produces more nuclear fuel than they use
breeder reactor
48
process of combining 2 nuclei to form a heavier nucleus
fusion
49
outermost shell of electrons
valence shell
50
what law states that elements show regular and repeating processes when they are arranged by their increasing atomic number
periodic law
51
each column of the periodic table is called a
group
52
each row of a period table is called
period
53
name given to group 1 of the periodic table
alkali metals
54
group 17
halogens
55
group 18
noble gases
56
3 general divisions of materials in the periodic table
metals, nonmetals, semimetals(aka metalloids)
57
groups of 2 or more atoms linked by chem bonds to form a distinct unit
molecule
58
molecules with same number and types of atoms but different arrangements
isomers
59
substance composed of atoms of two+ elements bonded together
compounds
60
substance with same physical property throughout and consists of one atom, molecule, or non molecular substance
pure substance
61
same physical property throughout
homogenous
62
physically mixed but not chemically united
mixture
63
what do we call homogenous mixture
solution
64
substance that gets dissolved
solute
65
mix containing tiny suspended clumps or particles
colloid
66
heterogeneous mix whose particles are large enough to settle
suspension
67
in a solution, what is the substance doing the dissolving
solvent
68
attractive forces holding atoms together
chemical bonds
69
of the 3 types of bonding, which type has the localized electrons across all atoms
metallic bonding
70
which bond is the sharing of electrons
covalent
71
what happens to electrons in ionic bonding
transferred
72
which type of covalent bond is the sharing of 4 electrons
double bond
73
electrons not centralized around a specific atom
delocalized electrons
74
diagram showing the location of all the atoms and valence electrons
lewis structure
75
ability of an atom to attract electrons to itself
electronegativity
76
when 2 elements of different electronegativity form a bond
polar bond
77
polar molecule has more electrons on one side
partial negative end
78
simplest ration of atoms in a covalent network
formula unit
79
addition of all the atomic masses of all the masses in a molecule
molecular mass
80
specific type of ion with more negative charge
anion
81
ionic bonding typically occurs btwn
a metal and a nonmetal
82
covalent bonding primarily forms between
2 nonmetals
83
an ion formed from a group of atoms
polyatomic ion
84
when naming covalent compounds, we use prefixes
true
85
when naming covalent substances, the second elements end of its name is changed to what
-ide
86
which formula allows chemists to represent the composition of a compound
chemical formula
87
type of formula telling how many of each type of atom are in a molecule
molecular formula
88
which type of formula shows the general arrangement of atoms in a molecule
structural formula
89
what formula shows the simplest ratio of atoms
empirical formula
90
what are the forces binding molecules together to form larger things
intermolecular forces
90
is C6H12 an empirical formula
no, because an empirical formula is the SIMPLEST ratio (it would be C1H2)
91
call the formula unit that specifies only the ratio of atoms or ions
unit cell
92
which intermolecular force occurs with H and nitrogen, oxygen, or fluorine
hydrogen bonding
92
which intermolecular force occurs across ALL molecules
London forces
93
knowing the methane is a non polar molecule whose chemical formula is CH4, what intermolecular forces are present in methane
london forces
94
water is a polar molecule and formula is h2o, which Im forces are present
hydrogen bonding, London forces, and dipole dipole forces
95
when molecules dissolve in a solvent, but ionic compounds
dissociate
96
general rule of thumb to determine if something will dissolve in something else
likes dissolve likes
97
what concentration is a measure of the moles of a solute per volume of solution
molarity
97
in general, if I increase temp what will happen to the rate of solution
it will increase
98
process of mixing the molecules of one substance with the molecules of another substance
diffusion
99
one way diffusion through a semipermeable membrane
osmosis
100
define insoluble
substance that does not readily dissolve in a given solvent
101
if I increase the temp of a gas, will it be more or less soluble
less soluble
102
molarity equation
moles of solute divided by liters of solution
103
molality equation
moles of solute divided by kilograms of solvent
