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A Level chemistry Y12 > 3.1.3. Bonding > Flashcards

3.1.3. Bonding Flashcards

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1
Q

What type of bonding exists between metals and non-metals?

A

Ionic bonding

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2
Q

What happens to electrons in ionic bonding?

A

They are transferred from metal to non-metal

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3
Q

Define ionic bonding

A

The electrostatic attraction between oppositely charged ions

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4
Q

Describe the structure of ionic compounds

A

Giant ionic lattice of positive and negative ions held together by electrostatic forces

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5
Q

Explain the melting point of ionic compounds

A

High melting point because strong electrostatic forces within ionic lattice

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6
Q

Explain the electrical conductivity of ionic compounds

A

Conduct when molten or dissolved because ions can move but do not conduct as a solid because ions held in fixed position in lattice

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7
Q

What happens to electrons in covalent bonding?

A

Electrons are shared between non-metal atoms

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8
Q

Define covalent bonding

A

The electrostatic attraction between the positively charged nucleus and the negative bonding pairs of electrons

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9
Q

What is the difference between a single and double covalent bond?

A

Single is 2 shared electrons in bond, double is 4 shared electrons

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10
Q

Describe the bonding in diamond

A

Each carbon is bonded to 4 other carbons in a tetrahedral shape

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11
Q

Describe the structure of graphite

A

Layers of carbon atoms arranged in hexagonal pattern with weak bonds and delocalised electrons between layers

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12
Q

Explain why graphite conducts electricity

A

Delocalised electrons are free to move and carry charge

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13
Q

Explain the hardness of diamond

A

Atoms are held in fixed positions

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14
Q

What is a co-ordinate (dative) bond?

A

Where one atom contributes both electrons in a covalent bond

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15
Q

Define metallic bonding

A

The electrostatic attraction between positively charged metal ions and the negatively charged sea of delocalised electrons

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16
Q

Describe the structure of metals

A

Giant metallic lattice of positive metal ions surrounded by delocalised electrons

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17
Q

How does the size of the ion affect melting point?

A

Increases with decreasing size

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18
Q

How does the charge of the ion affect melting point?

A

Increased with increasing charge

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19
Q

Explain why metals conduct electricity

A

Delocalised electrons are free to move and carry charge

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20
Q

Explain why metals have high melting points

A

The dleocalised electrons are strongly attracted to the positive metal ions (strong metallic bonds) which requires a lot of energy to overcome

21
Q

What is electron pair repulsion theory?

A

Electron pairs repel each other as far apart as possible.

22
Q

Which has the greater repulsion effect - lone pair of electrons or a covalent bond?

A

Lone pair

23
Q

What is the bond angle in a linear molecule?

A

180

24
Q

What is the bond angle in a trigonal planar molecule?

A

120

25
Q

What is the bond angle in a tetrahedral molecule ?

A

109

26
Q

What is the bond angle in a trigonal bipyramidal molecule?

A

120 and 90

27
Q

What is the bond angle in an octahedral molecule?

A

90

28
Q

What shape molecule has 6 bonding electron pairs, eg. SF6?

A

Octahedral

29
Q

What shape molecule has 5 bonding pairs eg. PCl5?

A

Trigonal bipyramidal

30
Q

What shape molecule has 4 bonding pairs eg. NH4+?

A

Tetrahedral

31
Q

What shape molecule has 3 bonding pairs eg. BF3?

A

Planar

32
Q

What shape molecule has 2 bonding pairs eg. BeF2?

A

Linear

33
Q

How do lone pairs affect bond angles?

A

Reduce bonding pair bond angles (by approx 2 degrees) as they repel more than bonding pairs

34
Q

What is the shape and bond angle in water? Why?

A

Bent, 104.5 degree, 4 pairs of electrons including 2 lone pairs

35
Q

Where in the periodic table are the most electronegative elements?

A

Top right (not including noble gases)

36
Q

Which is the most electronegative element?

A

Fluorine

37
Q

What causes bond polarity?

A

Differences in electronegativity between two atoms bonded together

38
Q

What causes molecule to be polar (2 requirements)?

A

Significant differences in electronegativity in atoms in the molecule, and asymmetrical shape

39
Q

Define electronegativity

A

The ability of an atom to attract electron density (the electron pair) in a covalent bond

40
Q

Name the 3 types of intermolecular force in order from weakest to strongest

A

Van der Waals, dipole-dipole and hydrogen bonding

41
Q

Explain how Van der Waals forces arise

A

Temporary dipoles because of movement of electrons which induce temporary dipoles in neighbouring molecules

42
Q

Explain how dipole dipole forces arise

A

Partial positive charge attracting partial negative charge

43
Q

Explain why generally boiling point increases with increasing chain length

A

More Van der Waals forces

44
Q

Describe the structure of iodine

A

Molecular lattice of I2 molecules held toegher by Van der Waals forces

45
Q

What 3 elements could be bonded to hydrogen to give hydrogen bonding?

A

Oxygen, nitrogen or fluorine

46
Q

What is a hydrogen bond?

A

An electrostatic force of attraction between an N, O or F atom and a hydrogen atom that is bonded to another N, O or F atom

47
Q

How does hydrogen bonding affect boiling point?

A

Increases boiling point

48
Q

Describe the structure of ice

A

Regular lattice strucutre of water molecules held tgether by hydrogen bonding. Less dense than water

A Level chemistry Y12 (8 decks)

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