Class 1 Flashcards
(90 cards)
1
Q
prefix - nano
A
10-9
2
Q
prefix - micro
A
10-6
3
Q
prefix - mili
A
10-3
4
Q
prefix - centi
A
10-2
5
Q
prefix - kilo
A
103
6
Q
prefix - mega
A
106
7
Q
angstrom
A
unit of length
10-10 m
8
Q
density formula
A
mass / volume
kg/m3 or g/cm3
9
Q
density of water
A
1 g/cm3
10
Q
empirical formula
A
reducing the molecular formula to the smallest possible ratio
11
Q
ammonium
A
NH4+
12
Q
hydronium
A
H3O+
13
Q
acetate
A
CH3CO2-
14
Q
bicarbonate
A
HCO3-
15
Q
cyanide
A
CN-
16
Q
hydroxide
A
OH-
17
Q
nitrate
A
NO3-
18
Q
nitrite
A
NO2-
19
Q
perchlorate
A
ClO4-
20
Q
carbonate
A
CO32-
21
Q
sulfate
A
SO42-
22
Q
sulfite
A
SO32-
23
Q
phosphate
A
PO43-
24
Q
what is a mole
A
6.02 x 1023 entities (Avogadro’s number)
25
how to calculate the # of moles
mass in grams / molecular weight
26
what is molarity
of moles of solute / # litres of solution
27
Law of Conservation of Mass
amount of mass does not change in a chemical reaction
28
limiting reagent
limits how much product a reaction can produce
29
group 1 metals oxidation state
+1
30
group 2 metals oxidation state
+2
31
fluorine oxidation state
-1
32
hydrogen oxidation states
+1 when bonded to something more electroneg. than carbon
-1 when bonded to something less electroneg. than carbon
0 when bonded to carbon
33
oxygen oxidation state
-2
34
oxygen's oxidation state exception in peroxides
-1 instead of -2
35
what never assumes a neg oxidation state
metals
36
what does a central nucleus contain
protons and neutrons (aka nucleons)
37
how are electrons held in the atom
by the electrostatic attraction of the positively charged nucleus
38
what is the atomic number
of protons in the nucleus of an atom
39
what is the atomic mass number
of neutrons + # of protons
40
what is an isotope
two atoms of the same element with a different # of neutrons
41
what is the atomic weight of an element
a weighted average of the masses of the element's isotopes
42
strong nuclear force
holds the protons + neutrons together in a nucleus
43
unstable nuclei are..
radioactive
44
radioactive decay
alternating the # of protons/neutrons or lowering of energy
45
alpha particle
2 neutrons + 2 protons
emitted from parent nucleus
46
types of beta decay
beta -
beta +
electron capture
47
characteristic of beta decay
conversion of a neutron into a proton
48
are beta or alpha particles more dangerous
beta - smaller + have more energy
49
beta - decay
too many neutrons: conversion of a neutron into a proton - ejected from the nucleus
atomic number is now 1 greater
mass number remains the same
50
which is the most common type of beta decay
beta -
51
beta + decay
too few neutrons: conversion of a proton → neutron and a positron
atomic number is now 1 less
mass number is the same
52
positron vs electron
positron is the electron's antiparticle
identical to electron but with a positive charge
53
electron capture
increase # of neutrons by capturing an electron from the closest electron shell & uses it to convert a proton into a neutron
atomic number is now 1 less
mass number is the same
54
gamma decay
when a nucleus relaxes to its ground state, it emits photons of electromagnetic radiation (aka gamma photons)
55
characteristics of gamma photons
very high frequency and energy
no mass or share
ejection from nucleus doesn't change the atomic number or mass number
56
half life equation
57
nuclear binding energy
energy that was released when the nucleons were bound together (by the strong force to form nucleus)
58
the greater the binding energy per nucleon..
the more stable the nucleus is
59
mass defect
when nucleons bind to form the nucleus, some mass is converted to energy so the mass of the combined nucleus is less than the sum of the nucleons masses
60
for a stable nucleus, the mass defect will always be..
positive
61
mass defect =
total mass of separate nucleons - mass of nucleus
62
Einstein & nuclear binding energy formula
63
energy of photon formula
64
absorption of a photon - energy change
positive energy change
65
emission of a photon - energy change
negative energy change
66
limitation of Bohr's model
only applies to atoms with only one electron
67
what is an orbital
a 3D region around the nucleus where electrons are most likely to be found
68
s subshell
one spherical orbital
69
p subshell
3 dumbbell shaped orbitals
70
Aufbau's principle
electrons occupy the lowest energy orbitals available
sub shells are filled in order of increasing energy
71
Hund's rule
electrons in the same subshell occupy available orbitals before pairing up
72
Pauli exclusion principle
no more than 2 electrons in any orbital
73
diamagnetic
an atom that has all of its electrons spin paired
no net magnetic field → will be repelled by a produced magnetic field
74
paramagnetic
when an atom's electrons are not all spin paired
attracted to externally produced magnetic fields
75
isoelectronic
when 2 atoms have the same electron configuration
76
atomic radius pattern
decreases across a period
increases down a group
77
ionic radius pattern
radius decreases as electrons are removed (cation)
radius increases as electrons are added (anion)
78
what is ionization energy
energy needed to remove an electron from an atom
79
ionization energy pattern
increases across a period
decreases down a group
80
what is electron affinity
amount of energy released when an electron is added
81
electron affinity pattern
electron affinity becomes more negative as we move across a period and up a row (except noble gases)
82
what is electronegativity
tendency for an atom to attract electrons
83
electronegativity pattern
increases across a period
decreases down a group
84
order of electronegativity
uncle F O N Cl
Br I S C H
85
what is acidity (trend)
how well a compound donates protons/excepts electrons
86
acidity pattern
increases across a period
increases down a group
87
number of protons =
atomic number
88
number of neutrons =
atomic mass - atomic number
89
Planck's constant
6.6 x 10-34 J.s
90
speed of light = c
3 x 108
