Key Concepts Flashcards

1
Q

What are spectator ions?

A

Ions that are unchanged in reactions

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2
Q

What is an ion?

A

A charged particle

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3
Q

What is an isotope?

A

Atoms of an element with the same number of protons but a different number of neutrons

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4
Q

How was Mendeleev’s version of the periodic table different to today’s version?

A

Some pairs of elements were the wrong way around (for example, iodine and tellurium), also there were gaps left for atoms that hadn’t yet been discovered

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5
Q

What is a cation?

A

A positively charged ion

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6
Q

What is an anion?

A

A negatively charged ion

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7
Q

What is the charge of a zinc ion?

A

2+

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8
Q

What is the charge of a copper ion?

A

2+

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9
Q

What is the charge of a silver ion?

A

1+

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10
Q

What are the possible charges of an iron ion?

A

2+ (II) 3+ (III)

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11
Q

What is the charge of an ammonium ion?

A

1+

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12
Q

What is the charge of a nitrate (NO3) ion?

A

1-

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13
Q

What is the charge of a sulfate ion?

A

2-

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14
Q

What is the charge of a carbonate(CO3) ion?

A

2-

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15
Q

What is the charge of a hydroxide ion?

A

1-

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16
Q

If ions have different numbers of charges what do you do to find out the formula of the compound that they form?

A

Times them together/ find the LCM

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17
Q

What are ionic bonds?

A

Strong electrostatic forces of attraction between oppositely charged ions

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18
Q

What structure do ionic compounds have?

A

Lattice structure which has a regular arrangement of ions

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19
Q

Do ionic compounds have high or low melting and boiling points?

20
Q

What state are ionic compounds in at room temperature?

21
Q

Are the majority of ionic compounds soluble or insoluble in water?

22
Q

What is a covalent bond?

A

A covalent bond is a bond between two atoms where a pair of electrons are shared between the two atoms

23
Q

What is a simple molecular substance?

A

Molecules consisting of only a few atoms

24
Q

What type of bonding do simple molecular substances have?

25
What state are simple molecular substances usually in at room temperature?
Liquid or gas
26
Do simple molecular substances have high or low melting and boiling points?
Low
27
What happens to the bonds/forces in simple molecular substances when they change state
The intermolecular forces are overcome but the covalent bonds do not break
28
Do simple molecular substances usually conduct electricity in solution?
No, however some simple molecular substances break down when in solution and form ions. The ions are free to move around so the solution conducts electricity (only when ions are formed)
29
Are simple molecular substances usually soluble in water?
No, they are usually insoluble because the intermolecular forces between the substance and the water are usually weaker than the intermolecular forces between the water molecules and between the molecules of the substance itself
30
When are simple molecular forces soluble?
When the simple molecular substance can form strong enough intermolecular forces with the water molecules
31
What is a giant molecular substance?
Molecules containing many atoms
32
What bonding do giant molecular substances have?
Covalent
33
What structure do giant molecular substances have?
Regular lattice structure
34
Do giant molecular substances usually have high or low boiling and melting points?
High
35
What state are giant molecular substances usually in at room temperature?
Solid
36
What type of model do you use to represent a giant molecule?
Ball and stick
37
Give some examples of giant molecular substances
- Graphite - Diamond - Graphene - Fullerenes
38
Why can graphene conduct electricity?
Non-bonding outer electrons become delocalised and are free to move through the structure
39
What structure do metals have?
Giant lattice of positively charged metal ions
40
What are metallic bonds?
Strong electrostatic forces of attraction between positively charged metal ions and delocalised electrons
41
Are metals usually soluble or insoluble in water?
Insoluble
42
What happens if a force is applied to a metal?
Layers of positively charged ions slide over each over and the metal changes shape without shattering
43
How do you calculate empirical formula?
- Divide the mass by relative formula mass - Divide both answers by the smallest answer - If there are fractions then multiply both answers to make sure there are no fractions
44
What is a closed system?
A situation where no substances can enter or leave during a reaction
45
What is a non-enclosed/open system?
A situation where substances can enter or leave during a reaction
46
What is the law of conservation of mass?
The mass of the reactants and products stays the same during a chemical reaction, the total mass of the substances involved is the same before and after a reaction
47
What does it mean when a reactant is in excess?
There will be some left over when the reaction is complete