Ions and Ionic bonding - 3rd

Question 1

what do metals tend to do to get a full outer shell?

Answer 1

metals tend to lose all of their outer-shell electrons to get a full outer-shell. this makes the charge of the ion positive.

Question 2

what is the loss of electrons called?

Answer 2

oxidation

Question 3

what is the gain of electrons called?

Answer 3

reduction

Question 4

what do non-metals tend to do to get a full outer shell?

Answer 4

metals tend to gain electrons to fill their outer-shell. this makes the charge of the ion negative.

Question 5

what does having a full outer shell do to the atom?

Answer 5

makes it more stable.

Question 6

what happens when metals and non-metals react?

Answer 6

the metal atoms give electrons to the non-metal atoms. every atom ends up forming an ion with a stable full outer-shell.

Question 7

draw and annotate an example of a metal and non-metal reaction?

Answer 7

ions and ionic bonding: picture 1

Question 8

what are the ion charges for different elements?

Answer 8

atoms in the same periodic table gain/lose the same number of electrons. this means that they form ions with the same charge ions and ionic bonding: picture 2

Question 9

how can you put ions together?

Answer 9

in an ionic compound, the charges balance : positive = negative.
we use subscript numbers to show how many of each ion must be present to make that work. in each compound, the total charge is zero.

Question 10

how are ions arranged?

Answer 10

in an ionic compound, the ions are arranged in a giant ionic lattice: ions and ionic bonding : picture 3

Question 11

define ionic bonding.

Answer 11

ionic bonding is the electrostatic attraction between oppositely charged ions. for example, in NaCl each Na + ion is attracted to the Cl - ions which surround it and vice-versa. ionic bonding is always a very strong attraction.

Question 12

do ionic compounds have high or low melting points?

Answer 12

high

Question 13

why do ionic compounds have high/low melting points?

Answer 13

ionic compounds have high melting points because:
- ionic bonds are very strong
- in a giant ionic lattice there are lots of ionic bonds
- breaking all the ionic bonds requires a large amount of energy.

Question 14

why do some ionic compounds have higher melting points?

Answer 14

some ionic compounds have higher melting points because their ions have higher charges. this makes the attraction between the ions even stronger and harder to break.

Question 15

what does electrical conductivity require?

Answer 15

charged particles which can move freely, which means that ionic compounds can only conduct electricity under certain circumstances.

Question 16

what is the conductivity in a solid and why?

Answer 16

no conductivity because ions can’t move freely.

Question 17

what is the conductivity in a liquid and aqueous and why?

Answer 17

high conductivity because ions can move freely.

Question 18

why do noble gases not readily react?

Answer 18

because they already have a full outer shell, which means that they are reluctant to share electrons.

Question 19

draw a dot and cross diagram for reacting lithium with oxygen.

Answer 19

ions and ionic bonding: picture 1

Question 20

what are the ionic charges for these transition metals:
- Ag
- Cu
- Fe
- Fe
- Pb
- Zn

Answer 20

• Ag +
• Cu 2+
• Fe 2+
• Fe 3+
• Pb 2+
• Zn 2+

Question 21

what are the ionic charges for these:
- hydrogen
- hydroxide
- ammonium
- carbonate
- nitrate
- sulfate

Answer 21

• hydrogen (H +)
• hydroxide (OH -)
• ammonium (NH4 +)
• carbonate (CO3 2-)
• nitrate (NO3 -)
• sulfate (SO4 2-)