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Chemistry > Intro to Gen Chem > Flashcards

Intro to Gen Chem Flashcards

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1
Q

Mass #

A

Protons + Neutrons (top number)

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2
Q

Atomic #

A

Protons (bottom number)

Determines identity

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3
Q

Isotope

A

Two or more atoms of same element but differing neutrons

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4
Q

Cation

A

protons > # e-

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5
Q

Anion

A

protons

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6
Q

Salt

A

Cation + anion

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7
Q

Periodic Table Trend: Atomic #

A

Increase L -> R

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8
Q

Non-metals

A

On the right, form anions (gain e-), use covalent bonds

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9
Q

Metals

A

On the left, form cations (lose e-), use ionic bonds

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10
Q

Metaloids

A

Makes up the border, some non-metal/metal qualities

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11
Q

Representative vs. Transition

A

1,2,13,14,15,16,17,18 vs 3,4,5,6,7,8,9,10,11,12

Ions by closest noble gas config. vs. lose e- from highest s subshell, then d-shell

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12
Q

Common Transition Metals

A

1+ ions: grp 11 Cu+, Ag+, Au+
2+ ions: most others
3+ ions: Cr 3+, Fe 3+, Au 3+, Al 3+, Bi 3+

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13
Q

Alkali Metal Characteristics

A 
Grp 1
Easily form 1+ cations (Na+)
Rxns: + nonmetals = ionic comp
\+ hydrogen = hydride
\+ water = metal hydroxide and H gas
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14
Q

Alkaline Earth Metal Characteristics

A

Grp 2

Form 2+ cations (Mg 2+)

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15
Q

Group 14

A

Form 4 covalent bonds with non-metals (2 more possible past 2nd period)
Only C forms strong pi-bonds

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16
Q

Group 15

A

Form 3 covalent bonds (2 additional past 2nd period, 1 additional w/ Lewis Base, N form it’s 4th by donating lone pair of e-)
N makes strong pi-bonds
P makes weak pi-bonds

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17
Q

Oxygen Group

A

Grp 16
Oxygen (O2 & O3): 2nd most electronegative, strong pi-bonds
Sulfur (S8): Can form 2-6 bonds, strong double bonds

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18
Q

Halogens

A

Grp 17
F, Cl, Br, I highly reactive
F only 1 bond

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19
Q

Nobel Gases

A

Grp 18

Non-reactive

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20
Q

Periodic Trends: Atomic Radius

A

Decreases left -> right (more protons pulling on e-)

Increases top -> bottom (outer e- being shielded)

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21
Q

Periodic Trends: Effective Nuclear Charge (Zeff)

A

Charge felt by most recently added e-
Increases left -> right
Increases top -> bottom (addition of shells)

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22
Q

Periodic Trends: Ionization Energy

A

Energy needed to detach an e- from an atom
Increases left -> right
Decreases top -> bottom (due to increased radius)

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23
Q

Periodic Trends: Electronegativity

A

Tendency of an atom to attract e- shared in covalent bond
Increases left -> right
Decreases top -> bottom
Large diff (1.6+) = ionic bond
Mod diff (0.5-1.5) = polar covalent bond
Minor diff (0-0.4) = non-polar covalent bond

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24
Q

Periodic Trends: Electron Affinity

A

Willingness of atom to accept additional e-
Increases left -> right
Decreases top -> bottom

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25
Q

Pauli-exclusion principle

A

No 2 e- can have same 4 quantum #s

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26
Q

Quantum Numbers

A

Principle, n, shell level
Azimuthal, l, subshell shape
Magnetic, ml, orbital w/in subshell
Spin, ms

27
Q

Heisenberg Uncertainty Principle

A

You don’t really know the position or momentum of a particle

28
Q

Subshell filling

A

s: grps 1,2
p: grps 13-18
d: 3-12

29
Q

Electron Configuration

A 
s   p    d   f
1  1s
2 2s 2p
3 3s 3p 3d
4 4s 4p 4d 4f
5 5s 5p 5d 5f
30
Q

Hund’s Rule

A

All orbitals in a subshell will contain 1 e- befroe filling any orbitals completely

31
Q

Photoelectric Effect

A

Demonstrates existance of 1:1 photon:e- collision

KE=hf - Φ

32
Q

Covalent Bond

A

e- shared between atoms, non-metals

33
Q

Ionic Bond

A

e- transferred from one atom to another

34
Q

Dipole Moment

A

When center of + charge doesn’t coincide with center of - charge, polar bond can be created

35
Q

H bond

A

Strongest dipole-dipole (H to F,O,N)

36
Q

London dispersion forces/Van der Waals

A

Between two instantaneous dipoles, weakest force

37
Q

Transition metal naming

A

Cation/anion followed by charge in Roman numeral

38
Q

Non-metal cation naming

A

Cation ends in -ium

39
Q

Non-metal anion naming

A

Simple end in -ide
multiple O end in -ite or -ate
hypo- and per- for more

40
Q

Ionic compound

A

cation + anion name (furthest left and lowest 1st)

2nd element ends in -ide

41
Q 
mega              micro
kilo                 nano
deci                pico
centi               femento
milli
A 
M 10^6            µ 10^-6   
k 10^3             n 10^-9
d 10^-1             p 10^-12
c 10^-2            f 10^-15
m 10^-3
42
Q

Empirical Formula

A

Smallest ratio of whole # used to represent molecule

43
Q

Molecular Formula

A

Exact # of elemental atoms

44
Q

Percent Composition by Mass

A

MW of 1 element’s atoms/MW of total atoms X 100%

45
Q

Finding Empirical Formula

A

x g element 1/ x atomic wt. = #x
y g element 2/ y atomic wt. = #y
#x/#y = ratio

46
Q

Combination Rxn

A

A+B->C

47
Q

Decomposition Rxn

A

C->A+B

48
Q

Single Displacement Rxn

A

A+BC->B+AC

49
Q

Double Displacement Rxn

A

AB+CD->AD+CB

50
Q

Redox Rxn

A

2Au 3+ + 3Zn ->2Au + 3Zn2+

51
Q

Combustion

A

C_6H_12 + 9O_2 -> 6CO_2 + 6H_20

52
Q

Theoretical Yield

A

Actual yield/theoretical yield x 100

53
Q

Moles

A

g/molecular weight

54
Q

Gram to Amu

A

1 g = 6.02x23 amu

55
Q

Kinetic vs Thermodynamic Control

A

Thermo:More stable, req higher nrg input, slow
Kinetic: Less stable, req lower nrg, faster

56
Q

Arrhenius Equation

A

k=Ae^(-Ea/RT) R=8.314J K^-1 mol^-1
Ea increase= rate constant decrease
catalysts increase rate constant by decreasing Ea
Temp increases rate constant
rms molecular velocity increases rate constant

57
Q

Rate Law

A

Rate=k[A]^α [B]^β

58
Q

Half life

A

A_t=A_o e^(-kt)

59
Q

Alpha Decay

A

Lose He nucleus,-4 in mass, -2 in Atomic #

60
Q

Beta Decay

A

Neutron -> proton, e- emitted, no change in mass, +1 in atomic #

61
Q

e- capture

A

Proton -> neutron, e- absorbed, no change in mass, -1 in atomic #

62
Q

Positron emission (Beta+)

A

Proton -> neutron, positron emitted, no change in mass, -1 in atomic #

63
Q

Gamma Decay

A

Neutron -> proton, e- emitted, no change in mass or atomic #

Chemistry (7 decks)

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