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Chemistry A-Level > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is ionic bonding

A

Electrostatic forces of attraction between oppositely charged ions in a lattice

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2
Q

Properties of ionic compounds

A

Solid at room temperature, giant lattice structure, conducts electricity when molten or dissolved, brittle

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3
Q

What is covalent bonding

A

A bond containing a shared pair of electron

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4
Q

What is a dative covalent bond

A

When the shared pair of electrons in a bond are supplied from one atom only

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5
Q

How is a dative covalent bond depicted

A

Using an arrow

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6
Q

Properties of covalent molecules

A

Low melting points due to the weak intermolecular forces of attraction, poor conductors of electricity

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7
Q

What is metallic bonding

A

Attraction between delocalised electrons and positive ions arranged in a lattice

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8
Q

What does the strength of a metal depend upon

A

Charge of the ion (more electrons in sea, stronger attraction) and size of the ion (nucleus closer to sea, stronger attraction)

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9
Q

Properties of metals

A

Good conductors of heat and electricity, malleable and ductile, high melting point, giant lattice

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10
Q

What is electronegativity

A

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

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11
Q

What does electronegativity depend upon

A

Nuclear charge, distance between the nucleus and outer electrons, shielding

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12
Q

Trend of electronegativity down a group

A

Less electronegative as larger distance from nucleus, more shielding, same nuclear charge

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13
Q

Trend of electronegativity across a period

A

More electronegative as larger nuclear charge, same distance from nucleus, same shielding

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14
Q

What occurs with electronegativity in a covalent bond

A

If there is a difference in electronegativity, this will produce a polar covalent bond. If the difference is too large, it will become a permanent dipole

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15
Q

The greater the difference in electronegativity…

A

The more polar is the covalent bond

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16
Q

What are the three intermolecular forces

A

Van der Waals forces, dipole-dipole forces and hydrogen bonding

17
Q

What are Van der Waals forces

A

The electrons at one instant may tend to be further on one side than the other, this creates a dipole causing other atoms to have the same

18
Q

What do Van der Waals affect

A

All atoms at all times

19
Q

What are dipole-dipole forces

A

When a molecule has a dipole bond, which attracts each other. If the dipoles are symmetrical they can cancel each other

20
Q

What is hydrogen bonding

A

Stronge intermolecular force between a bond hydrogen bond with a heavily positive charge attracted to another atom, with a heavily negative charge, with a lone pair

21
Q

Explain hydrogen bonding in ice

A

Water has hydrogen bond and when it freezes, the hydrogen bonds form and create a diamond-like structure. This has a lower density, causing ice to float on water, enabling fish to survive in winter

22
Q

What are the types of crystal structures

A

Ionic, metallic, macromolecular and molecular

23
Q

What are crystals

A

Crystals are solids with a regular arrangement of particles

24
Q

Describe ionic crystals with example

A

Strong electrostatic forces of attraction between oppositely charged ions such as sodium chloride. Attractions extend through the whole structure

25
Q

Describe metallic crystals with example

A

Attraction between lattice of positive ions and sea of delocalised electrons such as magnesium

26
Q

Describe molecular crystals

A

Intermolecular forces holding the covalent molecules together such as iodine. Large number of electrons so Van der Waals are strong enough to produce a solid crystal. But soft.

27
Q

Describe diamond

A

Macromolecular - covalent bonds between carbon atoms in 4 directions. Creating tetrahedral shape of 109.5 degrees. High melting point

28
Q

Describe graphite

A

Macromolecular - covalent bonds between carbon atoms in 3 directions. Shape of trigonal planar. Delocalised electrons. Weak intermolecular forces between layers. Conducts electricity but soft material

29
Q

How to draw hydrogen bonding

A

Dashed line, all charges, all lone pairs, 3 bonded atoms must be in a straight line, bond from lone pair to delta +

30
Q

What are the three elements that are electronegative enough to produce hydrogen bonding

A

Nitrogen, oxygen, fluorine

31
Q

Explain how dipole-dipole forces arise in hydrogen chloride

A

Difference in electronegativity produces a polarity, slightly negative charge from chlorine attracts the slightly positive charge from another hydrogen

Chemistry A-Level (34 decks)

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