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Ochem > Chapter 1 Book > Flashcards

Chapter 1 Book Flashcards

1
Q

Atoms

A

all matter is made of

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2
Q

describe an atom

A

Nucleus made of proton and neutrons and electron cloud surrounding nucleus

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3
Q

Atomic number

A

number of protons

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4
Q

Cation

A

+ charged with less electrons than protons

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5
Q

Anion

A
  • charged more electrons than protons
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6
Q

Isotopes

A

2 atoms of same element with different number of neutrons

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7
Q

Mass #

A

atoms total number of protons and neutrons in nucleus

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8
Q

Atomic weight

A

particular element weight from average mass of isotopes

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9
Q

What is the common H isotope and what is it called

A

1 proton with no neutrons is called deuterium

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10
Q

periodic table

A

schematic arrangement arranged by increasing atomic number

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11
Q

group number

A

column of periodic table

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12
Q

properties similar in columns and rows

A

similar size
similar electronic and chemical properties

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13
Q

orbitals and what are they named

A

region of space that is high electron density spdf

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14
Q

Shape of S orbital

A

sphere

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15
Q

Shape of P orbital

A

dumbell shape

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16
Q

Common bonds of atoms

A

H 1 bond
C 4 bonds
N 3 bonds 1 lone pair
O 2 bonds 2 lone pairs
X 1 bond 3 lone pairs

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17
Q

How many electrons can S orbital have

A

2

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18
Q

How many electrons can p orbitals have

A

6

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19
Q

Valence electrons

A

outmost electrons that bond to atoms

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20
Q

Compounds

A

2 or more elements

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21
Q

Octet rule

A

8 Valence electrons wanted

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22
Q

Ionic bonds

A

transfer of electrons to another element

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23
Q

Covalent bonds

A

sharing electrons between 2 nucei

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24
Q

What do ionic bonds form

A

crystal lattices

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25
Q

What bonds form molecules?

A

Covalent bonds

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26
Q

Lone pairs

A

unshared electrons

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27
Q

lewis structures

A

electrons dots representation for molecules

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28
Q

formal charge

A

charge assigned to single atoms in lewis structures

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29
Q

Formula for formal charge

A

of VE- (unshared electrons+ 1/2 of bond electrons)

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30
Q

Isomers

A

more than 1 arrangement of atoms possible from same molecular formula

31
Q

Constitutional isomers

A

same molecular formula but connectivity of atoms different

32
Q

exceptions to the octet rule

A

H has 2 electrons
B and Be not enough electrons
P and S more than 8 electrons

33
Q

resonance structures

A

2 lewis structures with same placement of atoms but different arrangement of electrons

34
Q

double-headed arrow

A

separates 2 resonance structures

35
Q

resonance hybrids

A

composite of both forms of resonance structures where electrons are delocalized and resonance stabilized

36
Q

curved arrow notation

A

shows how electron positions differ

37
Q

heteroatom

A

atom that is not C or H

38
Q

major contributor

A

better resonance structure

39
Q

minor contributor

A

not the better r structure

40
Q

What makes a resonance structure better

A

more bonds fewer charges

41
Q

Bond length

A

average distance between centers of 2 bonded nuclei

42
Q

how does bond length decrease and increase and why?

A

bond length decreases across row as size of atom decreases
bond length increases down a column as size of atom increases

43
Q

Bond angle

A

determines shape around any atom bonded

44
Q

VSEPR theory

A

electron pairs repel each other

45
Q

2 groups of electrons around atom

A

linear 180 degrees

46
Q

3 groups of electrons around atom

A

trigonal planar 120 degrees

47
Q

4 groups of electrons around atom

A

tetrahedral 109 degrees

48
Q

discuss lines on a molecule

A

solid line is in plane
wedge is in front of plane
dashed is behind plane

49
Q

trigonal pyramidal

A

tetrahedral with 1 lone pair 107 degrees

50
Q

Bent

A

tetrahedral 2 lone pairs 105 degrees

51
Q

condensed structures

A

All atoms bond lines omitted with parenthesis around similar groups with same atoms

52
Q

Skeletal structures

A

C is junction of 2 lines or at end of a line with C having enough H
draw all heteroatoms
charges take place of H with lone pairs

53
Q

sigma bond

A

cylindrically symetrical

54
Q

ground state

A

lowest energy arrangement

55
Q

hybridization

A

2 or more atomic orbitals form some # of hybrid orbitals

56
Q

sp3

A

2s1 and 2p3

57
Q

sp2

A

2s1 2p2

58
Q

sp

A

2s12p1

59
Q

pi bond

A

not concentrated on the axis and is weaker

60
Q

Bond length vs bond strength

A

increase in bond length= decrease in bond strength
decrease in bond length= increase in bond strength
therefore short bonds are strong bonds

61
Q

Joule

A

SI unit of energy

62
Q

Calories

A

O chem energy value unit

63
Q

Conversion of calories to Joules

A

1 cal= 4.18 J

64
Q

percent S character

A

fraction of hybrid orbital

65
Q

hybrid s characters percentage and why

A

sp is 1 2s/ 2 hybrid= 50% s characters
sp2 is 1 2s/ 3 hybrid= 33% s character
sp3 is 1 2s/ 4 hybrid= 25% s character

66
Q

What happens to electrons as % s character increases and what about the bonds

A

As % s character increases, hybrid holds elections closer causing bonds to become shorter and stronger

67
Q

Electronegativity and how it increases and decrease

A

measure of atoms attraction for electrons
increases across row of PT as nuclear charge increases
decreases down column of PT as atomic radius increases

68
Q

Where is most electronegative element

A

upper right hand corner

69
Q

dipole

A

partial sepration of charge

70
Q

Polar bond

A

electronegativity difference between 2 atoms is very small

71
Q

electrostatic potential map

A

distribution of electron density in a molecule where electron-rich area is red and electron-deficient is blue

72
Q

What type of polarity is H2O and why

A

Polar because O is different than Hs

73
Q

What type of polarity is CO2 and why

A

linear molecular cancels out polarity making it nonpolar

Ochem (10 decks)

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