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RSFC chemistry > 1.2 Bonding > Flashcards

1.2 Bonding Flashcards

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1
Q

Ammonium

A

NH4 +

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2
Q

Hydroxide

A

OH-

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3
Q

Nitrate

A

NO3 -

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4
Q

Nitrite

A

NO2 -

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5
Q

Hydrogencarbonate

A

HCO3 -

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6
Q

Chlorate (I)

A

ClO-

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7
Q

Chlorate (V)

A

ClO3 -

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8
Q

Carbonate

A

CO3 2-

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9
Q

Sulfate

A

SO4 2-

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10
Q

Sulfite

A

SO3 2-

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11
Q

Dichromate

A

Cr2O7 2-

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12
Q

Sulfide

A

S2-

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13
Q

Phosphate

A

PO4 3-

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14
Q

Nitride

A

N3-

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15
Q

Linear

A

180°

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16
Q

Trigonal planar

A

120°

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17
Q

Tetrahedral

A

109.5°

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17
Q

Tetrahedral

A

109.5°

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18
Q

Trigonal bipyramidal

A

120°
90°

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19
Q

Octahedral

A

90°

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20
Q

V-shape

A

2 bonding
1 lone
117.5°

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21
Q

Pyramidal

A

3 bonding
1 lone
107°

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22
Q

See-saw

A

4 bonding
1 lone
119
89

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23
Q

Square pyramidal

A

5 bonding
1 lone
89

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24
Q

V-shape

A

2 bonding
2 lone
104.5

25
Q

T-shape

A

3 bonding
2 lone
89

26
Q

Square Planar

A

4 bonding
2 lone
90

27
Q

Describe the structure and particles of metallic bonding

A

Structure: giant metallic lattice
Particles: positive metal ions
delocalised electrons

28
Q

Describe the structure and particles within ionic bonding

A

Structure: giant ionic lattice
Particles: negative and positive ions

29
Q

Describe the structure and particles of macromolecular covalent bonding

A

Structure: macromolecular
Particles: atoms

30
Q

Describe the structure and particles of simple molecular covalent bonding

A

Structure: simple molecular
Particles: molecules

31
Q

Metallic bonding definition

A

The strong electrostatic forces of attraction between positive metal ions and a sea of delocalised electrons

32
Q

Properties of metals

A

Conductivity: good electrical and thermal conductors
Strength: very strong
Malleable: highly malleable
Melting point: stronger the metallic bonds, the higher the melting or boiling point

33
Q

Why are metals good conductors?

A

The electrical current can be transferred through the delocalised electrons

34
Q

Why are most metals strong?

A

There is strong electrostatic forces of attraction between the metal ions and delocalised electrons

35
Q

Why are metals malleable?

A

The layers of metal ions can slide over each other

36
Q

What are the two types of covalent bonds?

A

Macromolecular
SImple molecular

37
Q

Covalent bond definition

A

A shared pair of electrons between two atoms

38
Q

Examples of macromolecular structures

A

Carbon
Silicon
Silicon oxide

39
Q

Ionic bonding definition

A

The strong electrostatic attraction between two oppositely charged ions

40
Q

How do you know what forms the positive or negative ion?

A

Electrons are transferred from the metal to the non metal
The metal will therefore always form the positive ion and the non metal will be negative

41
Q

Properties of ionic compounds

A

High melting point and boiling point
Electrical conductivity
Brittle

42
Q

Coordinate bond definition

A

A shared electron pair which both have come from there same atom

43
Q

How do you represent a covalent bond?

A

An arrow

44
Q

Electronegativity definition

A

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

45
Q

How does electronegativity change across the periodic table

A

Increases

46
Q

How does electronegativity change as you go down the periodic table

A

Decreases

47
Q

Why does the electronegativity change as you go across the periodic table?

A

The number of protons increases
Shielding stays the same
The ability to attract electrons in a covalent bond increases

48
Q

What are the types of intermolecular forces?

A

Induced dipole dipole
Permanent dipole dipole
Hydrogen bonding

49
Q

What type of IMF does a molecule have if it is polar?

A

Permanent dipole dipole

50
Q

What type of IMF does a molecule have if it isn’t polar?

A

Induced dipole dipole

51
Q

What does polar mean?

A
52
Q

What type of IMF is the strongest?

A

Hydrogen

53
Q

When does hydrogen bonding occur?

A

Between a H bonded to an O, N or F

54
Q

How does hydrogen bonding arise?

A

Large difference in electronegativity between the oxygen and hydrogen
This creates a dipole on the O-H
The lone pair on the oxygen atom in one molecule strongly attracts the partially positive hydrogen atom in another molecule

55
Q

When does PDD occur?

A

Between two polar molecules

56
Q

How does PDD arise?

A

Difference in electronegativity leads to bond polarity
Dipoles don’t cancel out therefore the molecule has an overall permanent dipole
There is an attraction between the delta positive on one molecule and the delta negative on another molecule

57
Q

When does IDD occur?

A

Between all molecules but generally non polar molecules

58
Q

How does IDD arise?

A

Random movement of electrons in one molecule leads to an
Uneven distribution of electrons creating a
Temporary dipole in one atom, this
Induces a dipole in a neighbouring molecule and
Dipoles attract

59
Q

When is hydrogen bonding used?

A

Ice
Proteins
DNA

RSFC chemistry (19 decks)

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