Chemistry A

Question 1

Where does Ionic bonding occur?

Answer 1

Between positive and negative ions, which attract each other and bind together to form ionic compounds.

Question 2

How is each ion held in place?

Answer 2

Each ion is surrounded by oppositely charged ions held in place by electrostatic attraction and forming a ionic crystal lattice.

Question 3

The ions in a crystal lattice….

Answer 3

are strongly bonded. A high temperature is required to melt the crystal.

Question 4

What happens during ionic bonding?

Answer 4

positive and negative ions attract one another and bind together forming a new substance.

Question 5

Where does covalent bonding occur?

Answer 5

It is formed between a non metal atoms

Question 6

What happens during covalent bonding?

Answer 6

Covalent bonding happens by sharing electrons.
The shared pair of electrons holds the two atoms together.

Question 7

Can covalent compounds conduct electricity?

Answer 7

they have no free electrons and no ions so they can’t conduct electricity.

Question 8

what diagrams show covalent bonding?

Answer 8

Dot and cross models show how a pair of electrons forms a covalent bond.

Question 9

where does metallic bonding occur?

Answer 9

In metal atoms

Question 10

What is metallic bonding?

Answer 10

Metallic bonding is the electrostatic attraction between positive metal ions and delocalised electrons.

Question 11

What are the melting/boiling points of metallic bonding?

Answer 11

metallic bonds are strong and a lot of energy is needed to break them. This is why metallic bonds have high melting and boiling points.

Question 12

how do metallic compounds conduct electricity?

Answer 12

metallic bonding is a strong attraction between closely packed positive metal ions and a “sea” of delocalized electrons. These electrons allow electricity to be carried.

Question 13

Do covalent compounds have high melting and boiling points?

Answer 13

The molecules of covalent compounds are held by weak intramolecular forces. Thus, a very small amount of energy is required to break the bonds between two or more molecules. That is why they have low melting and boiling points.

Question 14

Do ionic compounds have high melting and boiling points?

Answer 14

An ionic compound is a giant structure of ions. Ionic compounds are held together by strong electrostatic forces of attraction between oppositely charged ions. These compounds have high melting points and high boiling points because of the large amounts of energy needed to break the many strong bonds.

Question 15

what are the properties of group 0 metals?

Answer 15

they are called the noble gases. They are unreactive as they have a full outer shell. They don’t need to lose or gain any electrons.
They also have an increasing melting and boiling point going down the periodic table.

Question 16

what is an isotope?

Answer 16

Atoms of the same element with different numbers of neurons.

Question 17

what was Rutherfords gold foil experiment?

Answer 17

. Fired alpha particles at gold foil
. Most of the alpha particle went through, but a few were deflected
. this proved atomic structure was mainly empty space with small positively charged nucleus

Question 18

how did Mendeleev arrange the periodic table?

Answer 18

arranged by atomic mass and left gaps for undiscovered elements.

Question 19

how is the modern day periodic table arranged?

Answer 19

Elements are arranged by atomic number (proton number). Elements in the same group have similar chemical properties.

Question 20

properties of group 1 metals:

Answer 20

they are known as the alkali metals:
properties are:
- soft
- low melting/boiling point
- low density
- conducts electricity

Question 21

what happens when group 1 metals react with water?

Answer 21

• PH increases (more alkaline)
• fizzing/bubbling ( hydrogen is produced)
• metal becomes a sphere and floats on water
• produces a lilac flame

Question 22

what is the trend in reactivity in group 1?

Answer 22

Group 1 metals get more reactive going down the group. This is due to the outer electron being further away from the nucleus therefore weaker electrostatic attraction.

Question 23

what’s the appearance of group 7 metals?

Answer 23

fluorine: colourless gas
Chlorine: pale-yellow gas
Bromine: orange liquid
iodine: grey solid with purple vapour

Question 24

what the trend in physical properties? (group 7)

Answer 24

as you go down the group:
-colour gets darker
- boiling point increases

Question 25

what the trend in reactivity?
( group 7)

Answer 25

halogens get less reactive down the group. this is due to the outer electron shell being further away from the nucleus therefore weaker electrostatic attraction, electron is less easily gained.

Question 26

Do group 7 elements have a high melting/boiling point?

Answer 26

the boiling/ melting point increases going down the periodic table

Question 27

properties of transition metals:

Answer 27

• malleable
• hard
• high melting points
  -conduct electricity and heat