VSEPR and Types of Bonds

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2 electron groups, 0 lone pairs

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Chemistry

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1

2 electron groups, 0 lone pairs

e⁻ geo: linear molecular geo: linear hybridization: sp bond angle: 180°

<p>e⁻ geo: linear molecular geo: linear hybridization: sp bond angle: 180°</p>
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2

3 electron groups, 0 lone pairs

e⁻ geo: trigonal planar molecular geo: trigonal planar hybridization: sp² bond angle: 120°

<p>e⁻ geo: trigonal planar molecular geo: trigonal planar hybridization: sp² bond angle: 120°</p>
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3

3 electron groups, 1 lone pair

e⁻ geo: trigonal planar molecular geo: bent hybridization: sp² bond angle: <120°

<p>e⁻ geo: trigonal planar molecular geo: bent hybridization: sp² bond angle: &lt;120°</p>
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4

4 electron groups, 0 lone pair

e⁻ geo: tetrahedral molecular geo: tetrahedral hybridization: sp³ bond angle: 109.5°

<p>e⁻ geo: tetrahedral molecular geo: tetrahedral hybridization: sp³ bond angle: 109.5°</p>
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5

4 electron groups, 1 lone pair

e⁻ geo: tetrahedral molecular geo: trigonal pyramidal hybridization: sp³ bond angle: <109.5°

<p>e⁻ geo: tetrahedral molecular geo: trigonal pyramidal hybridization: sp³ bond angle: &lt;109.5°</p>
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6

4 electron groups, 2 lone pairs

e⁻ geo: tetrahedral molecular geo: bent hybridization: sp³ bond angle: <109.5°

<p>e⁻ geo: tetrahedral molecular geo: bent hybridization: sp³ bond angle: &lt;109.5°</p>
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7

5 electron groups, 0 lone pairs

e⁻ geo: trigonal bipyramidal molecular geo: trigonal bipyramidal hybridization: sp³d bond angle: 120° & 90°

<p>e⁻ geo: trigonal bipyramidal molecular geo: trigonal bipyramidal hybridization: sp³d bond angle: 120° &amp; 90°</p>
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8

5 electron groups, 1 lone pair

e⁻ geo: trigonal bipyramidal molecular geo: see saw hybridization: sp³d bond angle: <120° & <90°

<p>e⁻ geo: trigonal bipyramidal molecular geo: see saw hybridization: sp³d bond angle: &lt;120° &amp; &lt;90°</p>
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9

5 electron groups, 2 lone pairs

e⁻ geo: trigonal bipyramidal molecular geo: t-shaped hybridization: sp³d bond angle: <120° & <90°

<p>e⁻ geo: trigonal bipyramidal molecular geo: t-shaped hybridization: sp³d bond angle: &lt;120° &amp; &lt;90°</p>
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10

5 electron groups, 3 lone pairs

e⁻ geo: trigonal bipyramidal molecular geo: linear hybridization: sp³d bond angle: 180°

<p>e⁻ geo: trigonal bipyramidal molecular geo: linear hybridization: sp³d bond angle: 180°</p>
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11

6 electron groups, 0 lone pairs

e⁻ geo: octahedral molecular geo: octahedral hybridization: sp³d² bond angle: 90°

<p>e⁻ geo: octahedral molecular geo: octahedral hybridization: sp³d² bond angle: 90°</p>
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12

6 electron groups, 1 lone pair

e⁻ geo: octahedral molecular geo: square pyramidal hybridization: sp³d² bond angle: <90°

<p>e⁻ geo: octahedral molecular geo: square pyramidal hybridization: sp³d² bond angle: &lt;90°</p>
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13

6 electron groups, 2 lone pairs

e⁻ geo: octahedral molecular geo: square planar hybridization: sp³d² bond angle: 90°

<p>e⁻ geo: octahedral molecular geo: square planar hybridization: sp³d² bond angle: 90°</p>
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14

6 electron groups, 3 lone pairs

e⁻ geo: octahedral molecular geo: t-shaped hybridization: sp³d² bond angle: <90°

<p>e⁻ geo: octahedral molecular geo: t-shaped hybridization: sp³d² bond angle: &lt;90°</p>
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15

6 electron groups, 4 lone pairs

e⁻ geo: octahedral molecular geo: linear hybridization: sp³d² bond angle: 180°

<p>e⁻ geo: octahedral molecular geo: linear hybridization: sp³d² bond angle: 180°</p>
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16

ionic=

metal + nonmetal

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17

covalent=

non-metal + non-metal

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18

metallic

metals only

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19

ionic bond strength=

strong

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20

covalent bond strength=

weak

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21

metallic bond strength=

strong

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22

ionic is called...

compounds

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23

covalent is called...

molecule or molecular compound

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24

what happens to the electrons of ionics?

transfers electrons from metals to non-metals

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25

what happens to the electrons of covalents?

shares electrons (equally= non-polar, unequal= polar)

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26

what happens to the electrons of metallics?

delocalized (sea of electrons)

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27

ionic: formed from cations/anions?

made of cations (metal) and anions (non-metal)

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28

covalent: formed from cations/anions?

made only of anions

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29

metallic: formed from cations/anions

made only of cations

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30

ionic conductivity

conducts when dissolved in aqueous solution

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31

covalent conductivity

does NOT conduct electricity

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32

metallic conductivity

good conductors of heat and electricity

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33

ionic state of matter

solids at room temp (stronger bonds)

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34

covalent state of matter

liquids or gasses (weaker bonds)

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35

metallic state of matter

solids at room temperature

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36

ionic melting and boiling points

high

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37

covalent melting and boiling points

low

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38

metallic melting and boiling points

high

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39

ionic reason for forming a bond

forms a bond to become stable

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40

covalent reason for forming a bond

forms to become stable

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41

metallic reason for forming a bond

forms to become stable

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42

ionic characteristics include

brittle

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43

covalent characteristics include

network covalent

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44

network covalent

diamond and silicon are very strong bonds

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45

metallic characteristics include

shiny (luster), malleable/ductile

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46

ionic electronegativity values

high electronegativity difference

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47

covalent electronegativity values

low electronegativity difference

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48

metallic electronegativity values

low

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49

ionic bond energy

high

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50

covalent bond energy

low

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51

metallic bond energy

high

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52

ionic bond length

short

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53

covalent bond length

long

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54

metallic bond length

short

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55

Metallics have a short bond length because

electrons don't belong to any atom (= sea of electrons (delocalized))

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56

electricity=

flow of electric charges

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57

cations...

lose electrons and become positive (metals)

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58

anions...

gain electrons and become negative (non-metals)

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59

valence electrons...

involved in bonding and found in the outer most shell

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60

molecular orbit=

region in which shared electrons are found

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61

bond length=

average distance due to electrons moving in the form of a wave

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62

single bond length is

long

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63

single bond strength is

weak

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64

double bond length is

shorter than a single bond

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65

double bond strength is

stronger than a single bond

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66

triple bond length is

the shortest

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67

triple bond strength is

the strongest

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68

bond energy=

the amount of energy required to break the bond in 1 mole of a substance

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69

polar=

unequal sharing of electrons

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70

nonpolar=

equal sharing of electrons

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71

are diatomics polar or nonpolar?

always nonpolar

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72

polar=

opposites

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