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CHEMISTRY > GENCHEM > Flashcards

GENCHEM Flashcards

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1
Q

GAS TO SOLID PHASE CHANGE

A

DEPOSITION

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2
Q

ANYTHING THAT HAS MASS & VOL

A

MATTER

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3
Q

STATE OF MATTER THAT HAS PROTONS & NEUTRONS (affected by magnetic field)

A

PLASMA (ionized gas)

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4
Q

SIMPLEST FORM OF SUBSTANCE

A

ELEMENT

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5
Q

2 OR MORE ELEMENTS COMBINED & SEPARATED VIA CHM RXN

A

COMPOUND

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6
Q

COMPOSED OF 2 OR MORE SUBS WHICH IDENTITIES ARE RETAINED; VIA PHYSICAL MEANS

A

MIXTURE

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7
Q

TYPES OF MIXTURE

A

HOMOGENOUS & HETEROGENOUS MIXTURE

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8
Q

CLASSIFICATION OF SUBS BASED ON DEPENDENCE TO THE AMT OF MATTER PRESENT

A

EXTRINSIC & INTRINSIC

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9
Q

This law states that mass/matter is always constant (neither created nor destroyed)

A

LAW OF CONSERVATION OF MASS/MATTER

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10
Q

Proust’s Law

A

LAW OF DEFINITE PROPORTIONS

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11
Q

Proportions by wt. when chm rxn takes place can be expressed in small integral unit

A

LAW OF COMBININGI WEIGHTS

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12
Q

MODERN ATOMIC MODEL

A

Quantum mechanical/e-cloud

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13
Q

PLANETARY MODEL

A

Neil Bohr

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14
Q

Discovered PROTONS

A

Ernest Rutherford

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15
Q

Plum pudding/raisin bread model

A

JJ Thomson

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16
Q

Nuclear (Gold foil alpha scattering expt)

A

Ernest Rutherford

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17
Q

How to get # of neutrons?

A

PROTONS + NEUTRONS

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18
Q

How to get # of e-?

A

p+ in uncharged state - charge of element

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19
Q

How to get the charge of an element?

A

p+ - n

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20
Q

Eugen Goldstein

A

Discovered anode rays

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21
Q

Charge of ANODE

A

positive

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22
Q

Charge of CATHODE

A

negative

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23
Q

same p+, different element

A

ISOTOPES

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24
Q

ISOBARS

A

same atomic mass, different element

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25
Q

Give examples of non-isotopes

A

F, I, P

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26
Q

Examples of main isotopes

A

H, C, N, S, Cl, O, Br

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27
Q

same neutron, different element

A

ISOTONES

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28
Q

simplest whole # ratio

A

Empirical formula

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29
Q

Particle separation based on e#

A

Electrochemistry

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30
Q

Created by “molecule polarizibility” when 2 uncharged atom approach closely

A

Intermolecular/ Van der Waals/Electrostatic force of attraction

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31
Q

strongest type of intermolecular force of attraction

A

H-BONDING

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32
Q

weakest type of intermolecular force of attraction

A

London dispersion (ID-ID)

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33
Q

pair of valence e- that are not shared w/ another atom in covalent bond

A

Lone pair

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34
Q

What type of bond exhibits sharing of e- (nm + nm)?

A

COVALENT BOND

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35
Q

What type of bond exhibits transfer of e- (m + nm)?

A

IONIC BOND

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36
Q

Where bonds are formed by sharing an e- from overlapping atomic orbitals

A

VALENCE BOND THEORY

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37
Q

Predicts molecule’s geometry as well as any bonded & bonded e- pair?

A

VSEPR theory

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38
Q

Degree of tetrahedral/bent

A

109.5 °C

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39
Q

Where bonds are formed from the interaction of atomic orbitals from molecular orbitals

A

MOLECULAR ORBITAL THEORY

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40
Q

REACTION TYPES

A
  • Synthesis/combination/direct union
  • Decomposition/analysis
  • Single displacement
  • Double displacement
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41
Q

Give examples of covalent cmpds

A
  • CO
  • SiO2
  • N2O
  • CCl4
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42
Q

Give examples of ionic cmpds

A
  • Pb(NO3)4
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43
Q

Avogadro’s #

A

6.022x10^23 atom/molecule

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44
Q

Formula for Molarity (M)

A

M = n solute/ L soln

45
Q

Formula for Molality (m)

A

m = n solute / kg solvent

46
Q

Formula for Normality (n)

A

N = GEW/L or M x f

47
Q

Atoms may be built by progressive filling of energy of main energy sub level (lvls of lower energy lvls are occupied first

A

Aufbau principle

48
Q

Noble gas

A

He, Ne, Ar, Kr, Xe, Rn

49
Q

Serves as a fingerprint; unique for a particular element

A

QUANTUM NUMBERS

50
Q

Theory that states no two e- will have the same set of quantum #

A

Pauli’s Exclusion Theory

51
Q

BOYLE’S LAW FORMULA AND ITS CONSTANT

A

Constant = T

P1/V1=P2/V2

52
Q

CHARLE’S LAW FORMULA AND ITS CONSTANT

A

Constant = P

T1/V1=T2V2

53
Q

GAY LUSSAC’S LAW FORMULA AND ITS CONSTANT

A

Constant = V

P1/T1/=P2/T2

54
Q

COMBINED GAS LAW FORMULA

A

P1V1/T1=P2V2/T2

55
Q

AVOGADRO’S LAW FORMULA AND ITS CONSTANT

A

n = 6.02x10^23

V1/n1=V2/n2

56
Q

IDEAL GAS LAW FORMULA AND ITS CONSTANT

A 
R = 0.08205 univ gas constant
PV = nRT / P = MRT
57
Q

A gas law w/c states that a decrease in temp is an increase in P

A

HENRY’S LAW

58
Q

Formula to get °C

A

(F-32)/1.8

59
Q

Formula to get °F

A

(C x 1.8) + 32

60
Q

Formula to get K

A

C + 273.15

61
Q

Study of energy conversion/transformation in the univ

A

THERMODYNAMICS

62
Q

Law that states if 2 systems are in thermal equilibrium respectively with a 3rd system, they must be in thermal equilibrium w/ each other

A

ZEROTH LAW

63
Q

1ST LAW OF THERMODYNAMICS

A

LAW OF CONSERVATION OF ENERGY

64
Q

HESS’S LAW

A

ENTHALPHY (H) (heat/rxn energy)

65
Q

What rxn does +AH (enthalpy) exerts?

A

ENDOTHERMIC RXN

66
Q

What rxn does -AH (enthalpy) exerts?

A

EXOTHERMIC RXN

67
Q

Measure of a systems’ thermal energy per unit temp (disorderliness or randomness)

A

ENTROPY (S)

68
Q

What rxn does +AS (entropy) exerts?

A

SPONTANEOUS

69
Q

What rxn does -AS (entropy) exerts?

A

NON-SPONTANEOUS

70
Q

What rxn does -AG (gibb’s free energy) exerts?

A

SPONTANEOUS

71
Q

What rxn does +AG (gibb’s free energy) exerts?

A

NON-SPONTANEOUS

72
Q

Theory where in rxn rate is proportional to the # of collisions per time

A

COLLISION THEORY

73
Q

Theory where in the rate or rxn depends on the activation energy required to form intermediate/transition state

A

TRANSITION STATE THEORY

74
Q

FACTORS AFFECTING RXN RATE

A
  • Reactant’s nature
  • Surface area
  • Temp
  • Concentration
  • Catalyst
75
Q

States that rxn rate is proportional to the product of the conc. of reactants to the power of its coefficient in a balanced equation

A

LAW OF MASS ACTION

76
Q

EXTERNAL STRESSORS

A
  • Concentration
  • P
  • Vol
    Temp
  • Catalyst
77
Q

Used for hard soap manufacture

A

NaOH

78
Q

p+ donor

A

ACID

79
Q

e- donor

A

BASE

80
Q

Based on PEARSON’s HARD-SOFT ACID BASE concept, what is the thermodynamically stronger interaction?

A

Hard acid + Hard base

Soft acid + Soft base

81
Q

A phenomena that occurs when an ion is added in common w/ the subs already in equilibrium in the soln

A

COMMON ION EFFECT

82
Q

What resists pH change upon addition of small amts of either acid or base?

A

BUFFER SOLUTIONS

83
Q

Energy required to remove e- in a neutral atom?

A

IONIZATION POTENTIAl/ENERGY

84
Q

Energy released when neutral atom gains extra e- > more +

A

E- AFFINITY

85
Q

GROUP 1 A

A

ALKALI METALS

- H, Li, Na, K, Rb, Cs, Fr, NH4

86
Q

GROUP 2 A

A

ALKALINE EARTH M.

- Be, Mg, Ca, Sr, Ba, Ra

87
Q

GROUP 3A

A

BORON GRP

- B, Al, Ga, In, Tl

88
Q

GROUP 4A

A

CARBON GRP

- C, Si, Ge, Sn, Pb

89
Q

GROUP 5A

A

NITROGEN GRP

- N, P, As, Sb, Bi

90
Q

GROUP 6A

A

OXYGEN GRP

- O, S, Se, Te, Po

91
Q

GROUP 7A

A

HALOGENS

- F, Cl, Br, I, At

92
Q

GROUP 8A

A

NOBLE GAS

93
Q

GROUP 8A

A

NOBLE GAS

- He, Ne, Ar, Kr, Xe, Rn

94
Q

1B COINAGE M.

A
  • Cu, Ag, Au
95
Q

2B VOLATILE M.

A
  • Zn, Cd, hg
96
Q

3B SCANDIUM SUBGRP

A
  • Sc, Y, Lanthanides, Actinides
97
Q

4B TITANIUM SUBGRP

A
  • Ti, Zr, Hf
98
Q

5B VANADIUM SUBGRP

A
  • V, Nb, Ta
99
Q

6B CHROMIUM GRP

A

-Cr, Mo, W,

100
Q

7B MANGANESE SUBGRP

A

Mn, Tc, Re, Bh

101
Q

8B IRON TRIAD

A

1st: Fe, Co, Ni
2nd: Rh, Ru, Pd
3rd: Os, Ir, Pt

102
Q

Who discovered transuramic elements, greater than Uranium?

A

GLEEN SEABORG

103
Q

Discovered Po & Ra elements?

A

Marie Curie

104
Q

Discovered Uranium

A

Becquerel

105
Q

1 curie CI = ?

A

3.7x10^10 decay/sec

106
Q

Unit radiation damage

A

R.E.M

107
Q

Unit of amt of exposure to radiation

A

Rad/g = Gray

108
Q

Most penetrating ray/decay?

A

Gamma

109
Q

SOLID TO LIQUID PHASE CHANGE

A

MELTING

CHEMISTRY (5 decks)

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