Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Bonding (ionic) > Flashcards

Bonding (ionic) Flashcards

You may prefer our related Brainscape-certified flashcards:
Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards Periodic Table flashcards
1
Q

Define ionic bonding

A

The electrostatic forces of attraction between oppositely charged ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What charge ion does group 5, 6 and 7 atoms form?

A

Group 5 = -3 charge
Group 6 = -2 charge
Group 7 = -1 charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What charge ion do group 4 and group 0 atoms from?

A

Group 4 doesn’t have a charge
Group 0 has a charge of 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How are cations formed? Which elements tend to form cations?

A

Cations are formed by atoms losing electrons
Elements in groups 1,2 and 3 tend to lose electrons to form cations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the general equation for forming cations?

A

X ~> x ^n+ + xe-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What happens when atoms become ions?

A

They achieve stable noble gas configuration because the ions have full outer shells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How are anions formed?
What elements tend to form anions?

A

Anions are formed when atoms gain electrons to form positive ions
Elements in group 5 to 7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the general equation for forming anions? (Diatomic)

A

X2 + 2ne- ~> xn-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the valency number?

A

The valency number is the number on the charge of an ion without the positive or negative charge eg magnesium has a valency of 2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

How do you write formulas of ionic compounds using the valency method?

A

Write the each element and their charges
Use that to get their valency number
Cross the valencies
Write formula

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

How did you write formulas of ionic compounds using the balancing charges method?

A

Write each element and their charges
Calculate how many of each you would need to get overall charge of 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Why are Roman numerals used in the names of some metals?
Give an example

A

Some metals (usually in the d block) can form various ions so to identify which one it is the Roman numerals are used

For example Cu 2+ ions are Cu (II)
V 4+ ions are V (IV)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is a simple ion?
Give an example

A

An ion that is made from one element / atom eg Na

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is a polyatomic or complex ion?
Give an example

A

An ion that contains more than one type of atom, for example NH4+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are the 7 common polyatomic ions and their formulas?

A

Ammonium NH4+
Nitrate N03-
Hydroxide OH-
Hydrogensulfate HSO4-

Sulfate S042-
Carbonate CO32-
Phosphate PO4 3-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the rule for polyatomic ions and writing formulas?

A

If a polyatomic ion has a valency greater than 1 after swapping them then you must sue brackets

17
Q

Define an acid

A

A proton donor (H+)

18
Q

Why is aqueous HCl and acid but solid HCl isn’t?

A

Aqueous HCl is able to donate H+ ions because the water separates the H+ and Cl-

Solid HCl has particles held in a diced position so it cannnot donate a proton

19
Q

What does aqueous mean?

A

Dissolved in water

20
Q

What are the 5 common acids and their formulas?

A

Hydrochloric acid HCl
Sulfuric acid H2SO4
Nitric acid HNO3
Phosphoric acid H3PO4
Carbonic acid H2CO3

21
Q

What is a lattice?

A

A regular, repeated three dimensional arrangement of Jon’s / molecules or atoms in a solid

22
Q

What is a crystal structure?

A

A solid material whose constituents I.e molecules, atoms or ions are arranged in a highly ordered structure, forming a lattice that extends in all directions

23
Q

What are non crystalline structures called?

A

Amorphous

24
Q

How do you draw giant ionic lattices?

A

Draw a cube

Place an ion in the middle of each line

Place the opposite ion of the middle one in each corner

Place the same ion as the corner one on each side of the cube

25
Q

What is the melting and boiling point like in ionic compounds?

A

They have high melting and boiling points because there are strong electrostatic forces of attraction between the oppositely charged ions which require a lot of energy to break

26
Q

What are the 2 conditions for conductivity?

A

Delocalised ions
Delocalised electrons

27
Q

What is conductivity like in solid ionic compounds and why?

A

Solid ionic compound - don’t conduct electricity because the ions are held in the lattice structure so can’t move so can’t carry a charge

28
Q

What is conductivity like in molten ionic compounds and why?

A

They can conduct electricity as the ions are free to move so can carry a charge

29
Q

What is conductivity like in aqueous ionic compounds and why?

A

They can conduct electricity because the ions are separated by the water molecules so they are free to move so carry charge

30
Q

What makes water a polar molecule?

A

There is covalent bonding so both oxygen and hydrogen attempt to pull the electrons towards themselves. Oxygen has a higher electro negativity so it can pull the electrons closer which leaves it with a slight negative charge and hydrogen has a slight positive charge

31
Q

Why do atoms try to pull electrons towards themselves in covalent bonds?

A

To achieve greater stability

32
Q

How does water pull apart ions in solutions?

A

The delta plus and delta minus charge on hydrogen and oxygen can pull the ions apart by attracting them oppositely charged ones

33
Q

What ions are soluble and when? (4)

A

All NO3- compounds

All NH4+ , Na+ and K+ compounds

All Cl- , Br- and I- compounds

All SO42- compounds except with Ca2+ and strontium (Sr2+) and lead (Pb2+)

34
Q

What ions are insolubles and when? (2)

A

All CO32- (carbonate) compounds except with NH4+ ammonium , Na+ sodium and K+ potassium

All OH- (hydroxide) compounds except with NH4+ ammonium, Na+ sodium and K+ potassium

35
Q

What are 2 things that affect the strength of ionic bonds?

A

The ionic charge
The size of an ion

36
Q

How does the size of an ion change as you go down groups and accords periods?

A

Down = increase
Across = decrease

Chemistry (23 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions