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Chemistry 221 Final Exam > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

Ionic Bond

A

Metal Atom + Non-metal Atom, Transfer of electrons

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2
Q

Covalent Bond

A

Two Non-Metal Atoms, Sharing of Electrons

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3
Q

Perfect Covalent Bond

A

Two Identical Atoms

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4
Q

Polar Covalent Bond

A

Imperfect Sharing of Electrons, Partial Positive end and a Partial Negative end

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5
Q

Electronegativities

A

The closer the EN value between two electrons, the stronger the bond is

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6
Q

Lewis Structure

A

2-D representation of the connection between atoms

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7
Q

Octet Rule

A
  • 2nd row elements (C,N,O,F) = 8e-
  • Hydrogen = 2e-
  • 3rd row elements = (typically) 8e-
    Exceptions:
  • B and Al do not require an octet
  • S and P can have extended octets
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8
Q

Decrease of Unsaturation

A

U = (n(C) + 1) - 1/2(n(H) + X - n(N))
X = Halogens

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9
Q

of Valence e-

A

EX: C2H6O = 2(4) + 6(2) + 1(6) = 20e-

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10
Q

Formal Charge

A

Natural Bonding Pattern of an Atom
FC = (# Valence e-) - (Bonds + Lone e-)

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11
Q

Carbocation

A

Carbon with a positive formal charge

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12
Q

Carboanion

A

Carbon with a negative formal charge

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13
Q

Radical

A

a single unpaired electron

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14
Q

Resonance

A

The movement of electron to make or break double bonds to satisfy multiple unbalanced formal charges

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15
Q

Highest Contributing Resonance Form

A
  • All atoms have an Octet
  • Fewest Formal Charges
  • The atom carrying the FC is the most stable option
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16
Q

Bronsted Lowery Acid

A

Accepts e- (Donates a H+)

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17
Q

Bronsted Lowery Base

A

Donates e- (Accepts H+)

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18
Q

Common Strong Acids

A

H2SO4, HNO3, H3PO4

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19
Q

Acid Base Equilibrium Direction

A

Strong acid/base compounds react to make weak acid/base compounds - More than one trend shown leads you to look at the PKA

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20
Q

Equilibrium Direction (acid vs conj. acid or base vs conj. base) - Periodic trends

A

Larger atoms hold a negative charge better

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21
Q

Equilibrium Direction (acid vs conj. acid or base vs conj. base) - Electronegativity

A

Acid - the more electronegative atom is the stronger acid, more likely to stably hold extra electrons
Base - the more electronegative atom is the weaker base, wants to hold onto the electrons it has.

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22
Q

Equilibrium Direction (acid vs conj. acid or base vs conj. base) - Atom Size

A

Applies to atoms in the same column Larger atoms can hold the extra electrons over a larger area

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23
Q

Equilibrium Direction (acid vs conj. acid or base vs conj. base) - Induction

A

Distance of the most electronegative atom to the acidic hydrogen - The closer the electronegative atom is to the hydrogen the more pull it has on the electrons, thus weakening the O-H bond

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24
Q

Equilibrium Direction (acid vs conj. acid or base vs conj. base) - Hybridization

A

Electron density - Acidity = sp > sp2 > sp3

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25
Q

Equilibrium Direction (acid vs conj. acid or base vs conj. base) - Resonance

A

The more available resonance structures the weaker the base - electrons are shared across multiple atoms making it more stable

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26
Q

Equilibrium Direction (acid vs conj. acid or base vs conj. base) - pKa Values

A

Lower the pKa the more acidic - used when more than one acid/base indicator is present

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27
Q

Electrophile

A

Accepts e- (Acid)

28
Q

Nucleophile

A

Accepts a H+ (Base)

29
Q

Molecular Orbitals

A

Combination of atomic orbitals - # of atomic orbitals = # of molecular orbitals

30
Q

Bonding orbitals

A

Cunstructive/ Forms

31
Q

Anti-Bonding orbitals

A

Destructive/ Breaking

32
Q

Hybridization - sp3

A

sp3 -> 4 sp3 orbitals

33
Q

Hybridization - sp2

A

3 sp2 -> 3 sp2 orbitals + 1 empty p orbital

34
Q

Hybridization - sp

A

sp -> 2 sp orbitals + 2 empty p orbitals

35
Q

Special Derivatives - Methyl

A

Methyl Cation (sp2) - 3sp2 orbitals with an empty p orbital
Methyl anion (sp3) - 3 sp3 orbitals with a lone pair in a p orbital
Methyl Radical (sp2) - 3 sp2 orbitals with one e- in the p orbital

36
Q

Physical Properties of Polarity

A

BP, MP, and solubility are all determined by the dipole moment of the compound - stronger dipoles increase the energy needed to separate molecules from one another

37
Q

Intramolecular forces

A

Within a compund

38
Q

Intermolecular forces

A

Between molecules

39
Q

Atractive Forces

A

A. Charge - Charge, solids
B. Charge - Dipole, Solutions
C. Dipole - Dipole, polar liquids
D. Induced Dipole - Dipole, non-polar liquids

40
Q

Dipole - Dipole interaction

A

partial positives and partial negatives within a molecule interact with surrounding molecule’s partial positives and partial negatives

41
Q

Structural Isomers

A

made up of the identical atoms in a different arrangement - physical properties change

42
Q

Induced dipole - dipole interactions (LDF)

A

Temporary interactions created when non-polar molecules interact with one another - allows non-polar molecules to exist close together

43
Q

Shape’s affect on boiling point

A

The more surface area a molecule has the higher the boiling point - the more LDF’s that can be formed

44
Q

Bond Rotation

A

only single bonds can rotate freely - double bonds are fixed

45
Q

Isomerism

A

Different compounds with the same molecular formula

46
Q

Structural isomers

A

Same molecular formula but different connectivity

47
Q

Stereoisomers

A

Atoms connected in the same sequence but arranged differently in space - Cis/Trans isomers

48
Q

Wave number

A

identifies what bond is vibrating at that wavelength

49
Q

Finger print region

A

less than 1400 - unreliable

50
Q

Alkane sp3, R-C-H

A

Aprox. 2800 - 3000

51
Q

Alkene sp2, R=C-H

A

R=C-H Aprox. 3000 - 3100, C=C Aprox. 1640

52
Q

Alkyne sp

A

=_ C-H Aprox. 3300, C=_C-H Aprox. 2100

53
Q

Alcohols

A

Parabola Aprox. 3300

54
Q

Amines

A

N-H wide spike Aprox. 3300, NH2 double spike Aprox. 3300

55
Q

Ketone

A

C=O spike Aprox. 1700, no twin peak and no parabola

56
Q

Aldehyde

A

C=O spike Aprox. 1700 and twin beak C-H Aprox. 2700 and 2800

57
Q

Carboxylic Acid

A

Parabola with spikes out of the bottom Aprox. 3300 and C=O Aprox. 1700

58
Q

Amide

A

C=O Aprox. 1640-1680 and NH Aprox. 3300

59
Q

Nitriles

A

C=_N Aprox. 2200

60
Q

Esters

A

C=O Aprox. 1740 and C-O Aprox. 1100-1200

61
Q

Benzene

A

peak Aprox. 1600

62
Q

Mass Spec

A

M+ or M2+ can determine the compound with its mass

63
Q

Mass spec - Amines

A

odd M+

64
Q

Mass spec - Bromine

A

Twin peaks

65
Q

Mass spec - Chlorine

A

3/1 ratio M+/M2+

66
Q

Mass spec formula only C-H

A

M+ - ((M+/13)x12) = Hydrogens

Chemistry 221 Final Exam (5 decks)

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