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Ionic Bonding Flashcards

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1
Q

Rules for naming compounds containing a metal and a non-metal

A
  1. Metal is named first and keeps its name
  2. Non-metal ends in -ide
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2
Q

The formula of a compound tells us…

A
  1. Which elements are in the compound
  2. The ratio of each element present
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3
Q

Rules for naming a compound containing a metal, a non-metal and oxygen

A
  1. Metal name first
  2. Non-metal name + “ate” for the oxygen
    Eg. Magnesium Sulfate (MgSO4)
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4
Q

How to show numbers of atoms in compound names?

A

Mono = 1 (eg. carbon monoxide CO)
Di = 2 (eg. dihydrogen dioxide H2O2)
Tri = 3 (eg. sulfur trioxide SO3)
Tetra = 4 (carbon tetrachloride CCl4)

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5
Q

What are the diatomic molecules?

A

Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine

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6
Q

What is the most reactive element?

A

Fluorine

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7
Q

Gaining an ion description

A

Atoms take part in chemical reactions to achieve a full OUTER SHELL OF ELECTRONS, which is very stable (like noble gases). They can achieve this by either LOSING, GAINING or SHARING electrons from the outer shell. If an atom loses or gains electrons, the numbers of protons and electrons are no longer equal and a charged ION is formed. The charge on the ion depends on the number of electrons lost. Losing 1 electron results in a +1 ion. Losing 2 electrons results in a +2 ion.

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8
Q

Charged ions

A

Gaining electron = -
Losing electron = +

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9
Q

Ions in metals

A

Metal atoms achieve a full outer shell by losing electrons. Loss of electrons results in a positively charged ion: a CATION. The number of electrons lost, is the number of electrons in the outer shell of that atom.

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10
Q

Draw the calcium ion and electronic configuration

A

N/a

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11
Q

Ions in non-metals

A

Non-metal atoms achieve a full outer shell by gaining electrons. Gain of electrons results in a negatively charges ion: an ANION. The number of electrons gained, is the number of electrons required to get a full outer shell.

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12
Q

Forming compounds process

A

When a metal and non-metal react to form a compound, transfer of electron(s) from the metal atom to the non-metal atom occurs. An IONIC bond is formed, which is the electrostatic attraction between the positive cation and negative anion (oppositely charged ions).

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13
Q

Are ionic compounds neutral?

A

Yes, ionic compounds are neutral. This is because the positive ion charge cancels out the negative ion charge. The ratio of cation to anion is very important to ensure the positive and negative charges cancel.

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14
Q

State the formula of potassium oxide

A

K2O

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15
Q

Draw the dot and cross diagram of sodium oxide.

A

N/a

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16
Q

Why is hydrogen an exception?

A

Hydrogen has 1 electron in its outer shell, hence, it can lose or gain its outer electron.

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17
Q

What is the ion of silver?

A

Ag(+)

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18
Q

What is the ion of zinc?

A

Zn(2+)

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19
Q

What is the ion of lead?

A

Pb(2+)

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20
Q

What is the ion of iron (II)?

A

Fe(2+)

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21
Q

What is the ion of iron (III)?

A

Fe(3+)

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22
Q

What is the compound of aluminium oxide?

A

Al2O3

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23
Q

What is the compound of Iron (III) chloride?

A

FeCl3

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24
Q

Polyatomic meaning

Study These Flashcards
A

Ions that have many atoms / more than one atom

25
What is the polyatomic ion of hydroxide?
OH(-)
26
What is the polyatomic ion of carbonate?
CO3(2-)
27
What is the polyatomic ion of nitrate?
NO3(-)
28
What is the polyatomic ion of sulfate?
SO4(2-)
29
What is the polyatomic ion of ammonium?
NH4(+)
30
Polyatomic ion
Within a polyatomic ion, the non-metal atoms are chemically bonded together (by covalent bonds). It is the combined charge of all the atoms.
31
What is an ionic compound?
An ionic compound is a GIANT structure of ions. The ions have a regular repeating arrangement known as an ionic lattice. The lattice is formed due to the attraction between the ions, forming a regular pattern with oppositely charged ions next to each other.
32
Draw a 2D for an ionic compound
N/a
33
How big is the lattice?
The lattice is GIANT! One single grain of salt may contain 1.2 x 10^18 ions!
34
What is the ion of vanadium?
V(2+)
35
What is an ionic bond?
An ionic bond is the electrostatic force of attraction between a positively charged metal ion and a negatively charged non-metal ion.
36
What type of elements tend to react together to form ionic compounds?
Ionic compounds are formed from metallic elements with low electronegativity with non-metals that have a high electronegativity.
37
What is the ion of nitride?
N(3-)
38
What is the ion of lithium?
Li(+)
39
What is the ion of potassium?
K(+)
40
What is the ion of fluoride?
F(-)
41
What is the ion of bromide?
Br(-)
42
What is the ion of copper?
Cu(2+)
43
What is the ion of aluminium?
Al(3+)
44
What is the ion of chromium?
Cr(3+)
45
What is the ion of chloride?
Cl(-)
46
What is the ion of sulphide?
S(2-)
47
What are ions held together by?
Ions are held together by string electrostatic forces of attraction, which act between the oppositely charged ions.
48
When do ionic compounds conduct electricity?
When liquid or molten
49
Charge of Group 1 atoms?
+1
50
Charge of Group 2 atoms?
+2
51
Charge of Group 3 atoms?
+3
52
Charge of Group 5 atoms?
3-
53
Charge of Group 6 atoms?
2-
54
Charge of Group 7 atoms?
-
55
What is ionic bonding?
- A giant structure of ions = ionic compound - Held together by strong electrostatic forces of attraction between oppositely charged ions - The forces act in all directions in the lattice, and this is called ionic bonding.
56
Why do giant ionic lattices have high melting and boiling points?
Strong electrostatic forces of attraction between oppositely charged ions Requires a lot of energy to overcome these forces of attraction Therefore, the compounds have high melting and boiling points
57
Why do ionic compounds conduct electricity when aqueous or molten, but not when solid?
As a solid, the ions are in fixed positions so can't conduct electricity when molten or in aqueous solution the ions are free to move carrying charge and conducting electricity
58
What is lead iodide?
A solid

Chemistry (12 decks)

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