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3 bonding Flashcards

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1
Q

what type of ion does group 1 form?

A

1+

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2
Q

what type of ion does group 2 form?

A

2+

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3
Q

what type of ion does group 3 form?

A

3+

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4
Q

what type of ion does group 5 form?

A

3-

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5
Q

what type of ion does group 6 form?

A

2-

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6
Q

what type of ion does group 7 form?

A

1-

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7
Q

what is an ammonium ion?

A

NH4+

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8
Q

what is a hydroxide ion?

A

OH-

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9
Q

what is a nitrate ion?

A

NO3-

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10
Q

what is a nitrite ion?

A

NO2-

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11
Q

what is a hydrogencarbonate ion?

A

HCO3-

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12
Q

what is a chlorate (I) ion?

A

ClO-

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13
Q

what is a chlorate (V) ion?

A

ClO3-

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14
Q

what is a carbonate ion?

A

CO3^2-

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15
Q

what is a sulfate ion?

A

SO4^2-

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16
Q

what is a sulfite ion?

A

SO3^2-

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17
Q

what is a dichromate ion?

A

Cr2O7^2-

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18
Q

what is a phosphate ion?

A

PO4^3-

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19
Q

what is the shape of a molecule with 2 bonding pairs and 0 lone pairs called?

A

linear

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20
Q

what is the shape of a molecule with 3 bonding pairs and 0 lone pairs called?

A

trigonal planar

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21
Q

what is the shape of a molecule with 4 bonding pairs and 0 lone pairs called?

A

tetrahedral

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22
Q

what is the shape of a molecule with 5 bonding pairs and 0 lone pairs called?

A

trigonal bipyramidal

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23
Q

what is the shape of a molecule with 6 bonding pairs and 0 lone pairs called?

A

octahedral

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24
Q

what is the shape of a molecule with 2 bonding pairs and 1 lone pair called?

A

v-shaped

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25
Q

what is the shape of a molecule with 3 bonding pairs and 1 lone pair called?

A

pyramidal

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26
Q

what is the shape of a molecule with 4 bonding pairs and 1 lone pair called?

A

seesaw

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27
Q

what is the shape of a molecule with 5 bonding pairs and 1 lone pair called?

A

square pyramidal

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28
Q

what is the shape of a molecule with 2 bonding pairs and 2 lone pairs called?

A

v-shaped

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29
Q

what is the shape of a molecule with 3 bonding pairs and 2 lone pairs called?

A

trigonal planar

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30
Q

what is the shape of a molecule with 4 bonding pairs and 2 lone pairs called?

A

square planar

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31
Q

how many bonding pairs and lone pairs does a linear shaped molecule have?

A

2 bonding pairs
0 lone pairs

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32
Q

how many bonding pairs and lone pairs does a trigonal planar shaped molecule have?

A

3 bonding pairs
0 lone pairs
OR
3 bonding pairs
2 lone pairs

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33
Q

how many bonding pairs and lone pairs does a tetrahedral shaped molecule have?

A

4 bonding pairs
0 lone pairs

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34
Q

how many bonding pairs and lone pairs does a trigonal bipyramidal shaped molecule have?

A

5 bonding pairs
0 lone pairs

35
Q

how many bonding pairs and lone pairs does a octahedral shaped molecule have?

A

6 bonding pairs
0 lone pairs

36
Q

how many bonding pairs and lone pairs does a V shaped shaped molecule have?

A

2 bonding pairs
1 lone pair
OR
2 bonding pairs
2 lone pairs

37
Q

how many bonding pairs and lone pairs does a pyramidal shaped molecule have?

A

3 bonding pairs
1 lone pair

38
Q

how many bonding pairs and lone pairs does a seesaw shaped molecule have?

A

4 bonding pairs
1 lone pair

39
Q

how many bonding pairs and lone pairs does a square pyramidal shaped molecule have?

A

5 bonding pairs
1 lone pair

40
Q

how many bonding pairs and lone pairs does a square planar shaped molecule have?

A

4 bonding pairs
2 lone pairs

41
Q

what is the bond angle of a linear shaped molecule?

A

180

42
Q

what is the bond angle of a trigonal planar shaped molecule?

A

120

43
Q

what is the bond angle of a tetrahedralshaped molecule?

A

109.5

44
Q

what is the bond angle of a trigonal bipyramidal shaped molecule?

A

90
120

45
Q

what is the bond angle of a octahedralshaped molecule?

A

90

46
Q

what is the bond angle of a v shaped shaped molecule?

A

117.5
OR
104.5

47
Q

what is the bond angle of a pyramidal shaped molecule?

A

107

48
Q

what is the bond angle of a seesaw shaped molecule?

A

119
89

49
Q

what is the bond angle of a square pyramidal shaped molecule?

A

89

50
Q

what is the bond angle of a square planar shaped molecule?

A

90

51
Q

define metallic bonding

A

a strong electrostatic attraction of positive metal ions surrounded by a sea of delocalised electrons

52
Q

define ionic bonding

A

a strong electrostatic attraction between oppositely charged ions

53
Q

define covalent bonding

A

a shared pair of electrons between 2 atoms

54
Q

define dative covalent/coordinate bonding

A

a shared electron pair where both electrons come from the same atom

55
Q

what structure do metallic structures have?

A

giant metallic lattice

56
Q

what structures do ionic structures have?

A

giant ionic lattice

57
Q

what structure do covalent structures have?

A

macromolecular
OR
simple molecular

58
Q

what are 3 properties about metallic structures?

A

good thermal and electrical conductors
very strong
malleable and ductile

59
Q

what does the melting and boiling point depend on in metallic lattices?

A

strength of metallic bonds

60
Q

how do you find the stronger attraction of metallic bonds?

A

which has a greater charge
which has more electrons in the sea of delocalised electrons
which is smaller and therefore has more charge density

61
Q

which has a higher BP and MP? a molecule with a strong metallic bond or a molecule with a weak metallic bond?

A

strong

62
Q

what are 3 properties of ionic structures?

A

good electrical conductors
brittle
high melting and boiling point

63
Q

why are metallic structures malleable and ductile?

A

because layers of metal ions can slide past eachother

64
Q

what are 3 examples of things with macromolecular structures?

A

silicon
silicon oxide
carbon

65
Q

what are 2 examples of macromolecular crystals?

A

diamond
graphite

66
Q

describe the structure of diamond

A

macromolecular
each carbon has 4 covalent bonds
tetrahedral
high melting point
doesn’t conduct electricity

67
Q

describe the structure of graphite

A

macromolecular
each carbon has 3 bonds
separate layers held together with van de waals forces
high melting point
conducts electricity

68
Q

what are coordinate bonds represented with?

A

an arrow that goes from the atom that is donating the 2 electrons

69
Q

define electronegativity

A

the power of an atom to attract a pair of electrons in a covalent bond

70
Q

what determines electronegativity?

A

nuclear charge
atomic radius
shielding

71
Q

if an atom has high electronegativity it has…

A

high nuclear charge
low atomic radius
low amount of shielding

72
Q

what is the most electronegative atom?

A

fluorine

73
Q

what does non-polar mean?

A

an even distribution of electrons

74
Q

what does polar mean?

A

an uneven distribution of electrons

75
Q

what are the 3 types of inter molecular forces?

A

permanent dipole dipole
van de waals (induced dipole dipole)
hydrogen bonding

76
Q

what is the strongest inter-molecular force?

A

hydrogen bonding

77
Q

what is the weakest intermolecular force?

A

van de waals (induced dipole dipole)

78
Q

how do you find out whether a molecule has hydrogen bonding?

A

if there is a:
H-F
H-N
H-O

79
Q

how do you tell the difference between molecules with permanent dipole dipole forces and van de waals forces?

A

molecules with permanent dipole dipole forces are polar
molecules with van de waals forces are non polar

80
Q

the stronger an intermolecular force…

A

the more energy required to break the force
the higher the melting and boiling point

81
Q

how does hydrogen bonding arise?

A

very large difference in electronegativity between (atoms

creates a dipole on the (bond)

lone pair on ______ atom in one molecule STRONGLY attracts a ∂+H atom on a different molecule

82
Q

how do permanent dipole dipole forces arise?

A

difference in electronegativity leads to bond polarity

dipoles don’t cancel therefore the molecule has an overall permanent dipole

attraction between ∂+ on one molecule and ∂− on another

83
Q

how do van de waals forces arise?

A

random movement of electrons in one molecule leads to an

uneven distribution of electron, creating a

temporary dipole in one molecule. this

induces a dipole in a neighboring molecule

dipoles attract

chemistry (34 decks)

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