GENCHEM Flashcards
(109 cards)
1
Q
GAS TO SOLID PHASE CHANGE
A
DEPOSITION
2
Q
ANYTHING THAT HAS MASS & VOL
A
MATTER
3
Q
STATE OF MATTER THAT HAS PROTONS & NEUTRONS (affected by magnetic field)
A
PLASMA (ionized gas)
4
Q
SIMPLEST FORM OF SUBSTANCE
A
ELEMENT
5
Q
2 OR MORE ELEMENTS COMBINED & SEPARATED VIA CHM RXN
A
COMPOUND
6
Q
COMPOSED OF 2 OR MORE SUBS WHICH IDENTITIES ARE RETAINED; VIA PHYSICAL MEANS
A
MIXTURE
7
Q
TYPES OF MIXTURE
A
HOMOGENOUS & HETEROGENOUS MIXTURE
8
Q
CLASSIFICATION OF SUBS BASED ON DEPENDENCE TO THE AMT OF MATTER PRESENT
A
EXTRINSIC & INTRINSIC
9
Q
This law states that mass/matter is always constant (neither created nor destroyed)
A
LAW OF CONSERVATION OF MASS/MATTER
10
Q
Proust’s Law
A
LAW OF DEFINITE PROPORTIONS
11
Q
Proportions by wt. when chm rxn takes place can be expressed in small integral unit
A
LAW OF COMBININGI WEIGHTS
12
Q
MODERN ATOMIC MODEL
A
Quantum mechanical/e-cloud
13
Q
PLANETARY MODEL
A
Neil Bohr
14
Q
Discovered PROTONS
A
Ernest Rutherford
15
Q
Plum pudding/raisin bread model
A
JJ Thomson
16
Q
Nuclear (Gold foil alpha scattering expt)
A
Ernest Rutherford
17
Q
How to get # of neutrons?
A
PROTONS + NEUTRONS
18
Q
How to get # of e-?
A
p+ in uncharged state - charge of element
19
Q
How to get the charge of an element?
A
p+ - n
20
Q
Eugen Goldstein
A
Discovered anode rays
21
Q
Charge of ANODE
A
positive
22
Q
Charge of CATHODE
A
negative
23
Q
same p+, different element
A
ISOTOPES
24
Q
ISOBARS
A
same atomic mass, different element
25
Give examples of non-isotopes
F, I, P
26
Examples of main isotopes
H, C, N, S, Cl, O, Br
27
same neutron, different element
ISOTONES
28
simplest whole # ratio
Empirical formula
29
Particle separation based on e#
Electrochemistry
30
Created by "molecule polarizibility" when 2 uncharged atom approach closely
Intermolecular/ Van der Waals/Electrostatic force of attraction
31
strongest type of intermolecular force of attraction
H-BONDING
32
weakest type of intermolecular force of attraction
London dispersion (ID-ID)
33
pair of valence e- that are not shared w/ another atom in covalent bond
Lone pair
34
What type of bond exhibits sharing of e- (nm + nm)?
COVALENT BOND
35
What type of bond exhibits transfer of e- (m + nm)?
IONIC BOND
36
Where bonds are formed by sharing an e- from overlapping atomic orbitals
VALENCE BOND THEORY
37
Predicts molecule's geometry as well as any bonded & bonded e- pair?
VSEPR theory
38
Degree of tetrahedral/bent
109.5 °C
39
Where bonds are formed from the interaction of atomic orbitals from molecular orbitals
MOLECULAR ORBITAL THEORY
40
REACTION TYPES
- Synthesis/combination/direct union
- Decomposition/analysis
- Single displacement
- Double displacement
41
Give examples of covalent cmpds
- CO
- SiO2
- N2O
- CCl4
42
Give examples of ionic cmpds
- Pb(NO3)4
43
Avogadro's #
6.022x10^23 atom/molecule
44
Formula for Molarity (M)
M = n solute/ L soln
45
Formula for Molality (m)
m = n solute / kg solvent
46
Formula for Normality (n)
N = GEW/L or M x f
47
Atoms may be built by progressive filling of energy of main energy sub level (lvls of lower energy lvls are occupied first
Aufbau principle
48
Noble gas
He, Ne, Ar, Kr, Xe, Rn
49
Serves as a fingerprint; unique for a particular element
QUANTUM NUMBERS
50
Theory that states no two e- will have the same set of quantum #
Pauli's Exclusion Theory
51
BOYLE'S LAW FORMULA AND ITS CONSTANT
Constant = T
| P1/V1=P2/V2
52
CHARLE'S LAW FORMULA AND ITS CONSTANT
Constant = P
| T1/V1=T2V2
53
GAY LUSSAC'S LAW FORMULA AND ITS CONSTANT
Constant = V
| P1/T1/=P2/T2
54
COMBINED GAS LAW FORMULA
P1V1/T1=P2V2/T2
55
AVOGADRO'S LAW FORMULA AND ITS CONSTANT
n = 6.02x10^23
| V1/n1=V2/n2
56
IDEAL GAS LAW FORMULA AND ITS CONSTANT
```
R = 0.08205 univ gas constant
PV = nRT / P = MRT
```
57
A gas law w/c states that a decrease in temp is an increase in P
HENRY'S LAW
58
Formula to get °C
(F-32)/1.8
59
Formula to get °F
(C x 1.8) + 32
60
Formula to get K
C + 273.15
61
Study of energy conversion/transformation in the univ
THERMODYNAMICS
62
Law that states if 2 systems are in thermal equilibrium respectively with a 3rd system, they must be in thermal equilibrium w/ each other
ZEROTH LAW
63
1ST LAW OF THERMODYNAMICS
LAW OF CONSERVATION OF ENERGY
64
HESS'S LAW
ENTHALPHY (H) (heat/rxn energy)
65
What rxn does +AH (enthalpy) exerts?
ENDOTHERMIC RXN
66
What rxn does -AH (enthalpy) exerts?
EXOTHERMIC RXN
67
Measure of a systems' thermal energy per unit temp (disorderliness or randomness)
ENTROPY (S)
68
What rxn does +AS (entropy) exerts?
SPONTANEOUS
69
What rxn does -AS (entropy) exerts?
NON-SPONTANEOUS
70
What rxn does -AG (gibb's free energy) exerts?
SPONTANEOUS
71
What rxn does +AG (gibb's free energy) exerts?
NON-SPONTANEOUS
72
Theory where in rxn rate is proportional to the # of collisions per time
COLLISION THEORY
73
Theory where in the rate or rxn depends on the activation energy required to form intermediate/transition state
TRANSITION STATE THEORY
74
FACTORS AFFECTING RXN RATE
- Reactant's nature
- Surface area
- Temp
- Concentration
- Catalyst
75
States that rxn rate is proportional to the product of the conc. of reactants to the power of its coefficient in a balanced equation
LAW OF MASS ACTION
76
EXTERNAL STRESSORS
- Concentration
- P
- Vol
Temp
- Catalyst
77
Used for hard soap manufacture
NaOH
78
p+ donor
ACID
79
e- donor
BASE
80
Based on PEARSON's HARD-SOFT ACID BASE concept, what is the thermodynamically stronger interaction?
Hard acid + Hard base
| Soft acid + Soft base
81
A phenomena that occurs when an ion is added in common w/ the subs already in equilibrium in the soln
COMMON ION EFFECT
82
What resists pH change upon addition of small amts of either acid or base?
BUFFER SOLUTIONS
83
Energy required to remove e- in a neutral atom?
IONIZATION POTENTIAl/ENERGY
84
Energy released when neutral atom gains extra e- > more +
E- AFFINITY
85
GROUP 1 A
ALKALI METALS
| - H, Li, Na, K, Rb, Cs, Fr, NH4
86
GROUP 2 A
ALKALINE EARTH M.
| - Be, Mg, Ca, Sr, Ba, Ra
87
GROUP 3A
BORON GRP
| - B, Al, Ga, In, Tl
88
GROUP 4A
CARBON GRP
| - C, Si, Ge, Sn, Pb
89
GROUP 5A
NITROGEN GRP
| - N, P, As, Sb, Bi
90
GROUP 6A
OXYGEN GRP
| - O, S, Se, Te, Po
91
GROUP 7A
HALOGENS
| - F, Cl, Br, I, At
92
GROUP 8A
NOBLE GAS
93
GROUP 8A
NOBLE GAS
| - He, Ne, Ar, Kr, Xe, Rn
94
1B COINAGE M.
- Cu, Ag, Au
95
2B VOLATILE M.
- Zn, Cd, hg
96
3B SCANDIUM SUBGRP
- Sc, Y, Lanthanides, Actinides
97
4B TITANIUM SUBGRP
- Ti, Zr, Hf
98
5B VANADIUM SUBGRP
- V, Nb, Ta
99
6B CHROMIUM GRP
-Cr, Mo, W,
100
7B MANGANESE SUBGRP
Mn, Tc, Re, Bh
101
8B IRON TRIAD
1st: Fe, Co, Ni
2nd: Rh, Ru, Pd
3rd: Os, Ir, Pt
102
Who discovered transuramic elements, greater than Uranium?
GLEEN SEABORG
103
Discovered Po & Ra elements?
Marie Curie
104
Discovered Uranium
Becquerel
105
1 curie CI = ?
3.7x10^10 decay/sec
106
Unit radiation damage
R.E.M
107
Unit of amt of exposure to radiation
Rad/g = Gray
108
Most penetrating ray/decay?
Gamma
109
SOLID TO LIQUID PHASE CHANGE
MELTING
