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Organic Chemistry > Chapter 1 > Flashcards

Chapter 1 Flashcards

1
Q

define organic chemistry

A

chemistry of carbon compounds

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2
Q

define atomic numer

A

protons

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3
Q

define mass number

A

protons + neutrons

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4
Q

define isotope

A

same atomic number but differing neutrons

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5
Q

define valence electrons

A

electrons on the outermost shell

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6
Q

define the Aufbau principle

A

must fill the lowest energy orbitals first

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7
Q

define hunds rule

A

when there are two or more orbitals of the same energy, electrons will go into different orbital rather than pairing up in the same orbital

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8
Q

define ionic bonding

A
  • metal and a nonmetal
  • transferring of electrons
  • opposite charges attract
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9
Q

define covalent bonding

A
  • two or more nonmetals
  • electrons are charged
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10
Q

define non polar covalent

A

electrons are shared equally

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11
Q

define polar covalent

A

electrons are not shared equally
(one molecule is more electronegative)

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12
Q

formal charge equation

A

should - has

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13
Q

bonding pattern: Carbon

A

4 bonds

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14
Q

bonding pattern: Hydrogen

A

single

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15
Q

bonding pattern: Oxygen

A

2 bonds, 2 lone pairs

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16
Q

bonding pattern: Nitrogen

A

3 bonds, 1 lone pair

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17
Q

define sigma bond

A

a single bond

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18
Q

define a pi bond

A
  • double bond (1 pi bond)
  • triple bond (2 pi bonds)
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19
Q

define resonance forms

A

lewis structures that can be interconverted by moving electrons only

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20
Q

major resonance for criteria

A
  1. as many octets as possible
  2. as many bonds as possible
  3. charge on most electronegative atom
  4. same charge
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21
Q

Number of Carbons prefix: meth-

A

1

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22
Q

Number of Carbons prefix: eth-

23
Q

Number of Carbons prefix: pro-

24
Q

Number of Carbons prefix: but-

25
Q

Number of Carbons prefix: pent-

26
Q

Number of Carbons prefix: hex-

27
Q

Number of Carbons prefix: hept-

28
Q

Number of Carbons prefix: oct-

29
Q

Number of Carbons prefix: non-

30
Q

Number of Carbons prefix: dec-

31
Q

primary carbon

A

only attached to 1 carbon

32
Q

secondary carbon

A

attached to 2 carbons

33
Q

tertiary carbon

A

attached to 3 carbons

34
Q

define iso-

A

split on the end of a structure

35
Q

define sec-

A

attached to a secondary carbon

36
Q

define tert-

A

attached to a tertiary carbon

37
Q

define cis

A

on the same side of the molecule
(ex: 2 wedges)

38
Q

define trans

A

on opposite sides of the molecule
(ex: one wedge and one dash)

39
Q

rules of resonance: cations

A
  • 1 arrow
  • whole steps
  • arrows move bond to bond
40
Q

rules of resonance: anions

A
  • 2 arrows
  • 1/2 steps
  • arrows move bond to atom and atom to bond
41
Q

arrows go from ____ electron density to ____ electron density in resonance

42
Q

define VSEPR

A

Valence Shell Electron Pair Repulsion theory

43
Q

sp bond angle

44
Q

sp2 bond angle

45
Q

sp3 bond angle

46
Q

single bond and double bond rotation rules

A
  • single bond=allowed to rotate
  • double bond=CANNOT rotate
47
Q

what would make something more polar?

A

larger distance of electronegativity between atoms

48
Q

steps to determine hybridization

A
  1. count the number of atoms connected to the central atom
  2. count the number of lone pairs on the central atom
  3. add these values together
    - sp = 2
    - sp2 = 3
    - sp3 = 4
49
Q

define isomer

A

same molecular formula but differ in arrangement

50
Q

define constitutional isomer

A

differs in bonding sequence

51
Q

define stereoisomer

A

cis (same side) vs trans (opposite sides)

52
Q

why would isomers have the same mass?

A

because they have the same molecular formula

Organic Chemistry (9 decks)

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