Bonding Flashcards

1
Q

Which group rarely form bonds

A

The noble gases

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2
Q

How many types of bonding are there

A

3

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3
Q

What groups do ionic bonds occur between

A

Metals and non-metals

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4
Q

Electronegativity

A

The power/tendency of an atom to attract the electron density/ bonding pair in a covalent bond towards itself

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5
Q

First ionisation energy

A

The amount of energy required to remove one mole of electrons from one mole of gaseous atoms forming one mole of gaseous 1+ atoms

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6
Q

What groups do covalent bonds occur between

A

Non-metals only

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7
Q

How do ionic bonds work

A

One or more electron is stolen from the outer shell of the metal and then transferred over to the non-metal

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8
Q

Why does ionic bonding occur

A

So the electron orbitals can become as close to a noble gas as possible

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9
Q

What force attracts the ions together

A

Electrostatic forces

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10
Q

What structure do ions take up

A

Ionic lattices

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11
Q

Why are ionic lattices solid at room temperature

A

They are in a giant ionic lattice and thus have strong attraction in the lattice

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12
Q

Why are ionic substances brittle

A

They are alternating patterns of ions in a lattice shape. They shatter because they are unable to move past each other

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13
Q

What happens to the electrons in a covalent bond

A

They are shared between the atoms

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14
Q

Do covalent bonds carry charge

A

No as they are shared electrons and not transferred

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15
Q

How are covalent bonds held together

A

They are held together by electrostatic attraction between the nuclei and the shared electrons

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16
Q

What is the difference between a double and single covalent bond

A

In single 1 pair of electrons are shared
In double 2 pairs of electrons are shared

17
Q

What is it called when a covalent molecule accepts another atom

A

Co-ordinate/dative bonds

18
Q

What does metallic bonding occur between

A

Metal atoms

19
Q

What happens to the electrons in a metallic bonding

A

They become delocalised

20
Q

Which bonds are usually broken first

A

The weakest bond (the lowest bond enthalpy)

21
Q

What affects the electronegativity

A

Nuclear charge
Distance between electron and outer shell
Atomic shielding

22
Q

In relation to electronegativity, the smaller the atom,….

A

The closer the nucleus is to the outer electrons and is more electronegative

23
Q

In relation to electronegativity
The larger the nuclear charge for a given shielding effect …

A

The greater the electronegativity

24
Q

What is a polar bond

A

It is the unequal sharing of the electron between atoms that are covalently bonded

25
Q

What happens to polarity when 2 identical atoms bond

A

They form a non-polar bond

26
Q

What happens when 2 different atoms covalently bond

A

The electrons will be pulled towards the more electronegative atom

27
Q

How is polarity represented

A

δ- or δ+

28
Q

What is the weakest intermolecular force

A

Van der waals forces

29
Q

What is the average strength intermolecular force

A

Dipole-dipole force

30
Q

What is the strongest intermolecular force

A

Hydrogen bonding

31
Q

How do dipoles work in molecules

A

Dipoles can cancel if it is mirrored eg linear molecules

32
Q

Dipole- dipole forces act on what

A

They act on molecules with permanent dipoles

33
Q

How do van der waals forces work

A

It’s electrostatic attraction between the temporary dipoles caused by the electron “orbits”

34
Q

What do van der waals forces act on

A

All atoms or molecules at all times

35
Q

What affects the probability of van der waals forces

A

Having more electrons

36
Q

What is hydrogen bonding

A

When a hydrogen atom gets “sandwiched” between 2 very electronegative atoms forming a strong bond

37
Q

What are the conditions required for hydrogen bonding

A

A hydrogen atom that is bonded to a very electronegative atom forcing it to be partly positive
A very electronegative atom with lone pairs

38
Q

What are the atoms able to form hydrogen bonds

A

Oxygen,nitrogen,fluorine