Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chem 2070 > Basic terms and things to remember > Flashcards

Basic terms and things to remember Flashcards

(101 cards)

Start Studying
1
Q

Formal Charge

A

va- - bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

frequency

A

v= c/ Landon

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

azimuthal quantum

A

-can be a whole # b/t 0 and n-1
-determines shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Magnetic quantum number(ml)

A

-any whole # b/w -l and +l

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

change in energy

A

2.179*10^-18 (1/nf ^2 / 1/ni ^2)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

principle quantum number (n)

A

-can be any whole number greater than 1
-called shells
-indicates size or radius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

orbital vs. value of l

A

value of l orbital
0 s
1 p
2 d
3 f

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

covalent bonds

A

an electron spends some time around one atom and some time around a different atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

ionic bonds

A

an electron is fully transferred from one atom to another

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

paramagnetic

A

has at least one unpaired electron, attracted to external magnetic fields

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Diamagnetic

A

has all electrons paired

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Electron pair geometry

A

2-linear
3-trigonal planar
4-tetrahedral
5-trigonal bipyramidal
6-octahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Magnetic spins (ms)

A

-spin of an electron
-can be +1/2 or -1/2
[upwards and downwards arrows respectively]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Formal charge part 2

A

of va- - # of lone pair electrons - (1/2 * # of bonding e-)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Nitrite

A

Formula: NO2 -
Charge: 1-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Nitrate

A

Formula:NO3-
Charge:1-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Ammonium

A

Formula: NH4+
Charge: 1+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Cyanide

A

Formula: CN-
Charge: 1-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Carbonate

A

Formula: CO3
Charge: 2-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Visible light

A

400 nm(violet) - 700 nm(red)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

kinetic energy

A

Ek= hv(irridated) - hv(threshold)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Sulfite

A

Formula: SO3
Charge: 2-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Sulfate

A

Formula:SO4
Charge:2-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Phosphate

A

Formula: PO4
Charge: 3-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Hydroxide
Formula: OH Charge: 1-
26
ALWAYS soluable
N itrates (NO3) A cetates (C2H3O2) G roup 1 (Li,Na,etc.) S ulfates (SO4) A mmonium (NH4) G roup 17 (F, Cl,etc.)
27
Exceptions to solubility
P lead M mercury S silver [never soluble with sulfates] Ca Sr Ba (CastroBear)
28
Combustion
a substance CxHy reacts with oxygen to produce carbon dioxide and water CxHy +O2 --> H2O +CO2
29
pH Formula
pH= -log [H3O+] 10^-pH =[H3O+]
30
Double displacement
The metals trade, which non-metal they are associated with
31
proton
+1
32
elecron
-1
33
Neutron
0
34
Ion
atom or group of atoms that contain a charge
35
Atomic symbol of element
a X z a: mass (protons +neutrons) X: chemical symbol z: atomic
36
Isotopes
atoms of the same element that differ in atomic mass (neutrons differ)
37
Average atomic mass
(abundance % * Mass 1) + (abundance % * mass 2)...
38
Formula mass
sum of individual atoms in a substance (also called Formula weight)
39
Empirical Formula
lowest ratio of atoms in a compound
40
% yield
= actual yield/ theoretical *100
41
Limiting reagant
consumed completely during reaction
42
Homogenous mixture
Combine 2 components that cannot be easily separated
43
Molarity
M = mol/ Liters
44
Heterogenous mixture
combine 2 components that can be easily separated
45
concentration changes when volume changes
M1V1=M2V2
46
Lewis Acid
electron acceptor (metal cation)
47
Lewis Base
electron donor
48
Bronstead acids
H+ donor (HCl)
49
Bronstead Bases
H+ acceptor (NaOH)
50
Bases
produces OH- in solution
51
Acidity
pH= -log[H+]
52
Base pH equation
pOH= -log[OH-]
53
Dipole moment
separation of charge
54
Spectator ions
ions not engaged in overall reaction
55
Reduction
gain e-, charge decreases
56
Oxidation
lose e-, charge increases
57
e- donor
reducing agent/reductant
58
e- acceptor
oxidizing agent/ oxidant
59
Disproportionation
same substance is being oxidized and reduced
60
Decomposition
when a substance splits into smaller substances
61
Niels Bohr postulates
-atoms have discrete energies - atoms are in stationary orbits --> e- didn't collapse into nucleus - changes in E = hv (radiation emitted/ absorbed leadsto state change) - quantum conditions will be used
62
Radial function
-no angular dependence -amplitude -tells us size of orbital
63
Angular function
tell us shape of orbital
64
Pauli exclusion principle
you cannot have 2 e- in the same direction (spin) in one orbital
65
Aufbav principle
e-s are filled in lower energy orbitals before higher energy levels
66
Hund's rule
e-s have to fill at least once in every subshell before adding to the second
67
Full or half filled shells
MORE STABLE
68
Core e-s
any e-s that are not valence e-s ; unreactive in comparison to va e-'s
69
Valence e-s
outer shell e-s
70
Orbital vs. subshell e-s
Orbital subshell e-s s 2 p 6 d 10 f 14
71
As Zeff goes up
covalent radius goes down
71
Slater's rule
calculate zeff for any electron of interest
71
Zeff
effective nuclear charge
71
Ionization energy
energy required to remove an e- from an atom
71
Electron affinity
opposite of ionization energy (ability of atom to accept an e-)
72
Electronegativity
ability of an atom to attract an e- [highest EN = F!!]
73
Cations shrink covalent radii
zeff increases, orbitals contract, radius decreases
74
Anions expand covalent radii
zeff decreases, orbitals expand, radius increases
75
Steric number
SN = number of lone e- pairs on central atom + bonds
76
VSPER geometry
SN Geometry 1 linear 2 linear 3 trigonal planar 4 tetrahedral 5 trigonal bipyramidal 6 octahedral
77
SN 3 other geometries
lone pair name 0 trigonal planar 1 bent 2 linear
78
SN 4 other geometries
lone pair name 0 tetrahedral 1 trigonal pyramidal 2 bent
79
SN 5 other geometries
lone pair name 0 trigonal bipyramidal 1 seesaw 2 t-shaped 3 bent
80
SN 6 other geometries
lone pair name 0 octahedral 1 square pyramidal 2 square pyramidal 3 t-shaped 4 bent.
81
SN # vs. Hybridization
SN Hybridization 1 s 2 sp 3 sp^2 4 sp^3 5 sp^2 6 sp
82
Ideal gas law
PV=nRT P: pressure V: volume n: moles R: constant T: temperature (in K)
83
radioactive decay
spontaneous decomposition of nuclide
84
alpha particle
4 [alpha symbol] 2
85
beta particle
0 B -1
86
half life equation
t 1/2 = ln (2)/ K
87
finding concentration?? (1/2)
ln (nt /no) = -kt
88
cations
positive charge
89
Anions
negative charge
90
Left side of the periodic table
-"early elements" -tend to lose e- -Reactivity increases as you go down
91
Right side of the periodic table
-tend to gain e- -"late elements" -Reactivity decreases as you go down
92
Chemical equation approach
-identify compounds that have unique elements -adjust balancing coefficients so that # of atoms of each Z match -Leave H and O for lasts -use fractions if necessary
93
Algebraic chemical equation approach
-each substance gets a variable -Consider each element -start making assumptions -put these numbers back into the equation -multiply whole equation to obtain integer values
94
Simple reactivity
-group 1--> exists as +1 cation (except hydrogen) -group 2--> +2 cations - group 3--> +3 cations - group 16--> -2 anions -group 17 --> -1 anions -group 18 (noble gases) --> NO REACTIVITY
95
Equation
moles = x grams of substance / formula mass g/mol substance
96
Empirical formula approach
- assume 100g of substance - convert to moles - divide all amounts by smallest amount mol value
97
a strong acid will have a
weak conjugate base

Chem 2070 (2 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions