Intro to Gen Chem Flashcards

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
Pauli-exclusion principle
No 2 e- can have same 4 quantum #s
26
Quantum Numbers
Principle, n, shell level Azimuthal, l, subshell shape Magnetic, ml, orbital w/in subshell Spin, ms
27
Heisenberg Uncertainty Principle
You don't really know the position or momentum of a particle
28
Subshell filling
s: grps 1,2 p: grps 13-18 d: 3-12
29
Electron Configuration
``` s p d f 1 1s 2 2s 2p 3 3s 3p 3d 4 4s 4p 4d 4f 5 5s 5p 5d 5f ```
30
Hund's Rule
All orbitals in a subshell will contain 1 e- befroe filling any orbitals completely
31
Photoelectric Effect
Demonstrates existance of 1:1 photon:e- collision | KE=hf - Φ
32
Covalent Bond
e- shared between atoms, non-metals
33
Ionic Bond
e- transferred from one atom to another
34
Dipole Moment
When center of + charge doesn't coincide with center of - charge, polar bond can be created
35
H bond
Strongest dipole-dipole (H to F,O,N)
36
London dispersion forces/Van der Waals
Between two instantaneous dipoles, weakest force
37
Transition metal naming
Cation/anion followed by charge in Roman numeral
38
Non-metal cation naming
Cation ends in -ium
39
Non-metal anion naming
Simple end in -ide multiple O end in -ite or -ate hypo- and per- for more
40
Ionic compound
cation + anion name (furthest left and lowest 1st) | 2nd element ends in -ide
41
``` mega micro kilo nano deci pico centi femento milli ```
``` 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
Empirical Formula
Smallest ratio of whole # used to represent molecule
43
Molecular Formula
Exact # of elemental atoms
44
Percent Composition by Mass
MW of 1 element's atoms/MW of total atoms X 100%
45
Finding Empirical Formula
x g element 1/ x atomic wt. = #x y g element 2/ y atomic wt. = #y #x/#y = ratio
46
Combination Rxn
A+B->C
47
Decomposition Rxn
C->A+B
48
Single Displacement Rxn
A+BC->B+AC
49
Double Displacement Rxn
AB+CD->AD+CB
50
Redox Rxn
2Au 3+ + 3Zn ->2Au + 3Zn2+
51
Combustion
C_6H_12 + 9O_2 -> 6CO_2 + 6H_20
52
Theoretical Yield
Actual yield/theoretical yield x 100
53
Moles
g/molecular weight
54
Gram to Amu
1 g = 6.02x23 amu
55
Kinetic vs Thermodynamic Control
Thermo:More stable, req higher nrg input, slow Kinetic: Less stable, req lower nrg, faster
56
Arrhenius Equation
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
Rate Law
Rate=k[A]^α [B]^β
58
Half life
A_t=A_o e^(-kt)
59
Alpha Decay
Lose He nucleus,-4 in mass, -2 in Atomic #
60
Beta Decay
Neutron -> proton, e- emitted, no change in mass, +1 in atomic #
61
e- capture
Proton -> neutron, e- absorbed, no change in mass, -1 in atomic #
62
Positron emission (Beta+)
Proton -> neutron, positron emitted, no change in mass, -1 in atomic #
63
Gamma Decay
Neutron -> proton, e- emitted, no change in mass or atomic #