Bonding Flashcards

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
Describe metallic crystals with example
Attraction between lattice of positive ions and sea of delocalised electrons such as magnesium
26
Describe molecular crystals
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
Describe diamond
Macromolecular - covalent bonds between carbon atoms in 4 directions. Creating tetrahedral shape of 109.5 degrees. High melting point
28
Describe graphite
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
How to draw hydrogen bonding
Dashed line, all charges, all lone pairs, 3 bonded atoms must be in a straight line, bond from lone pair to delta +
30
What are the three elements that are electronegative enough to produce hydrogen bonding
Nitrogen, oxygen, fluorine
31
Explain how dipole-dipole forces arise in hydrogen chloride
Difference in electronegativity produces a polarity, slightly negative charge from chlorine attracts the slightly positive charge from another hydrogen