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
What happens to polarity when 2 identical atoms bond
They form a non-polar bond
26
What happens when 2 different atoms covalently bond
The electrons will be pulled towards the more electronegative atom
27
How is polarity represented
δ- or δ+
28
What is the weakest intermolecular force
Van der waals forces
29
What is the average strength intermolecular force
Dipole-dipole force
30
What is the strongest intermolecular force
Hydrogen bonding
31
How do dipoles work in molecules
Dipoles can cancel if it is mirrored eg linear molecules
32
Dipole- dipole forces act on what
They act on molecules with permanent dipoles
33
How do van der waals forces work
It’s electrostatic attraction between the temporary dipoles caused by the electron “orbits”
34
What do van der waals forces act on
All atoms or molecules at all times
35
What affects the probability of van der waals forces
Having more electrons
36
What is hydrogen bonding
When a hydrogen atom gets “sandwiched” between 2 very electronegative atoms forming a strong bond
37
What are the conditions required for hydrogen bonding
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
What are the atoms able to form hydrogen bonds
Oxygen,nitrogen,fluorine