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Chemical Reactions & Equations Flashcards

1
Q

Macroscopic observations that indicate a chemical change:

A
  • gas production
  • temperature change
  • colour change
  • new odour
  • formation of bubbles or precipitation
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2
Q

What is a chemical reaction?

A

A chemical reaction is a chemical change where at least one new substance is formed. It is often difficult to reverse.

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3
Q

What are atoms?

A

The smallest unit of an element that can take part in a reaction. They are spherical and so small they are invisible.

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4
Q

What is a molecule?

A

Any particle made up of two or more atoms.

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5
Q

Description of an element

A

Pure, consists of one type of atom. They cannot be simplified.

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6
Q

Description of a compound

A

Pure, made up of two or more elements chemically bonded in a fixed ratio by mass.

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7
Q

Hydrochloric acid

A

HCL

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8
Q

Sulfuric acid

A

H2SO4

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9
Q

Nitric acid

A

HNO3

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10
Q

Carbonic acid

A

H2CO3

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11
Q

Metal carbonate ➡️

A

Metal oxide + carbon dioxide

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12
Q

What is an acid?

A
  • any compound, that when dissolved in water, produces hydrogen ions
  • contain hydrogen, sour, corrosive, turn litmus red, turn universal indicator red, orange or yellow.
  • pH
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13
Q

What is a base?

A
  • any compound, that when dissolved in water, produces hydroxide ions
  • bitter, corrosive, turn litmus blue, turn universal indicator purple or blue
  • pH > 7
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14
Q

What are metal salts?

A
  • any compound that is made up of metal atoms bound to non-metal atoms
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15
Q

State the Law of Conservation of Mass

A

The Law of Conservation of Mass says that mass is neither created nor destroyed but conserved during chemical reactions.

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16
Q

Characteristics of non-metals:

A
  • typically brittle
  • quite hard to mold into different shapes
  • cannot conduct hear or electricity
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17
Q

Characteristics of metals:

A
  • generally shiny, malleable, and hard

- they are good conductors of electricity and heat

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18
Q

Characteristics of metalloids:

A
  • share characteristics of both metals and non-metals
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19
Q

What is an alkali?

A

Bases that dissolve in water

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20
Q

What is an isotope?

A

An atom of an element with a different number of neutrons.

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21
Q

Metal + oxygen ➡️

A

Metal oxide

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22
Q

Metal oxide + water ➡️

A

Metal hydroxide

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23
Q

What are valence electrons?

A

The electrons in the outer energy level

24
Q

Period number

A

Indicates number of energy levels in an atom

25
Group number
Indicates number of balance electrons in an atom
26
What is the octet rule?
8 electrons = chemical stability
27
Valency
Valency is the number of valence electrons an atom had to lose or gain to become chemically stable.
28
Polyatomic ions
Polyatomic ions are ions made up of two or more atoms. Groups of atoms joined together with a charge on the group.
29
Hydroxide
OH
30
Nitrate
NO3 1
31
Ammonium
NH4 1
32
Sulfate
SO4 2
33
Carbonate
CO3 2
34
Phosphate
PO4 3
35
Exothermic reactions
Chemical reactions that give out energy. This energy comes from the re-arrangement of atoms.
36
Endothermic reactions
Chemical reactions that absorb energy. They absorb energy from their surroundings.
37
Ionic bonding
Compete transfer of valence electrons from a metal atom to a non-metal atom results in the formation of a cation and an anion. Electrostatic attraction between ions form iconic bonds resulting in an ionic compound.
38
Characteristics of ionic compounds:
- they are made up of positive and negative ions - they are usually solids at room temperature - they normally have a high melting points because the electrostatic force of attraction between the ions is very strong - they usually dissolve in water to form aqueous solutions
39
What is a lattice?
A lattice is an ordered structure of ions held together by the electrostatic attraction between the positive and negative ions and is the basis to crystal formation.
40
Non-metal + oxygen ➡️
Non-metal oxide
41
Non-metal oxide + water ➡️
Acid
42
Outline a physical change
A physical change can be easily reversed. No new substances are formed.
43
What is a reactant?
A substance that takes part in and undergoes change during a reaction
44
What is a product?
The result of a reaction
45
Why are most elements on earth found in compounds?
The atoms of most elements are chemically reactive, that is, when they come into contact with certain other elements, they react with each other to form compounds.
46
Non-metal atoms
Gain electrons and becomes a negatively charged particle = ANION
47
Metal atoms
Lose valence electrons and becomes positively charged ions = CATIONS
48
Outline ionic bonding
A complete transfer of valence electrons from a metal atom to a non-metal atom resulting in the formation of cations and anions.
49
How are ionic compounds formed?
The electrostatic attraction between the two ions forms chemically binds them together to form an ionic compound.
50
Outline covalent bonding
The sharing of valence electron pairs between non-metal ions in order to attain a stable electronic configuration.
51
How are covalent compounds formed?
The electrostatic attraction of positively and negatively charged areas between atoms results in a covalent bond.
52
Characteristics of covalent compounds
- they exist as gases, liquids or solids with low melting points because the forces between molecules are relatively weak - they generally do not conduct electricity because they are not made up of ions. - they are usually insoluble in water
53
What does a covalent molecular formula indicate?
It indicates how many of atom covalently join together to form a discrete molecule. The covalent bonds holding atoms together within a molecule are strong but the forces between molecules are weak.
54
Acid + base ➡️
Metal salt + water
55
Metal oxide + water ➡️
Metal hydroxide
56
Acid + metal oxide ➡️
metal salt + water

Chemistry (2 decks)

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