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Chemistry (JW) > 2.2.2 Bonding and Structure > Flashcards

2.2.2 Bonding and Structure Flashcards

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1
Q

isoelectronic

A

same electron configuration

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2
Q

cation and anion

A

cation = positive ion, anion= negative ion

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3
Q

Name and explain properties of ionic structures (3)

A

High melting point: strong electrostatic attraction

Brittle: when moved, like charged ions repel

Electrical conductivity: not as solid- fixed in giant ionic lattice structure, do molten or aqueous- ions free to move and carry charge

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4
Q

2 reasons for ionic compounds having different boiling and melting points

A

1) charge on ions- e.g 2+ and 2- attract more strongly than 1+ and 1-
2) size of ions- smaller ions get closer together and so electrostatic attractions are greater

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5
Q

Structure of ionic compounds and reasons why

A

Giant ionic lattice.

Maximises attraction and minimises repulsion.

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6
Q

Covalent Bonds

A

Two non-metals sharing a pair of electrons to form structures isoelectronic to noble gases.

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7
Q

How do covalent bonds stay together?

A

Electrons attracted to positive nucleus of adjacent atoms. (electrostatic attraction)

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8
Q

average bond enthalpy

A

degree of strength a covalent bond has/ amount of energy to break bond (kJ mol-1)

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9
Q

dative (co-ordinate) bond

A

A covalent bond in which both electrons come from same atom.

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10
Q

How is a co-ordinate bond shown in simple diagrams?

A

With an arrow pointing from the atom donating the lone pair to the atom accepting it.

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11
Q

electron deficient

A

Atoms or molecules that have fewer than the number of electrons required for maximum stability.

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12
Q

Why are covalently bonded molecules poor electrical conductors?

A

No ions to move the electrical charge.

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13
Q

Why do simple covalent compounds have low melting points?

A

Although covalent bonds are strong, intermolecular forces are weak so need little energy to be overcome.

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14
Q

Showing 3D arrangement in diagrams (3 types of lines)

A

ordinary line= bond in plane of paper
dotted line= bond going away into paper
wedge= bond coming out towards you

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15
Q

Why does H2O have a bond angle of 104.5?(2)

A
  • electron pairs repel

- lone pairs repel more

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16
Q

2 bond pairs, 0 lone pairs

A

linear

180 degrees

17
Q

2 bond pairs, 2 lone pairs

A

non- linear

104.5 degrees

18
Q

3 bond pairs, 0 lone pairs

A

trigonal planar

120 degrees

19
Q

3 bond pairs, 1 lone pair

A

trigonal pyramidal

107 degrees

20
Q

4 bond pairs, 0 lone pairs

A

tetrahedral

109.5 degrees

21
Q

5 bond pairs, 0 lone pairs

A

trigonal bipyramidal

90 and 120 degrees

22
Q

6 bond pairs, 0 lone pairs

A

octahedral

90 degrees

23
Q

electronegativity

A

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

24
Q

What element has the highest electronegativity?

Which two have the lowest?

A

Fluorine - 4.0

Caesium and Francium - 0.79

25
Q

What is the electronegativity of noble gases? Why?

A

0 because they have full valence shells

26
Q

Explanation for electronegativity patterns in the periodic table

A

LESS DOWN GROUP: More shells between nucleus and outer shell, so more shielding and not as good at pulling electrons
MORE ACROSS PERIOD: increasing nuclear charge has stronger pull on electrons

27
Q

polar bond

A

Covalent bond in which there is a separation of charge between one end and the other.

28
Q

permanent dipole

A

molecule with two poles

29
Q

Is CO2 polar ? Why?

A

No. It is symmetrical so the dipoles cancel each other out.

30
Q

Ionic bonds can show covalency if…

A

1) positive ion is small and highly charged.

2) negative ion is large (=highly polarisable)

31
Q

Charge density equation

A

Charge density = charge of the ion/ionic radius

32
Q

Polarising ability increases as …

A

1) positive ion gets smaller

2) number of charges gets larger

33
Q

intermolecular forces/attractions are…

A

attractions between one molecule and a neighbouring molecule

34
Q

intramolecular forces are…

A

forces within molecules

35
Q

attraction that occurs between polar molecules which have a permanent dipole is called…

A

permanent dipole/ permanent dipole attraction

36
Q

Two things needed for hydrogen bonding to occur

A

1) must be attached to one of N, O, or F (these have high electronegativity
2) must be a lone pair of electrons on the electronegative atom

37
Q

What type of bonding is hydrogen bonding?

A

It is a special case of permanent dipole/ permanent dipole attraction.

38
Q

How would you draw hydrogen bonding in water?

A

Water molecule in non-linear shape.

Hydrogen bond between hydrogen and lone pair of electrons on oxygen in an adjacent molecule.

Chemistry (JW) (3 decks)

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