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Chemistry > C3 - Atoms, elements and compounds > Flashcards

C3 - Atoms, elements and compounds Flashcards

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1
Q

Define an element [2]

A
  • Made of a single type of atom
  • Cannot be broken down into smaller parts
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2
Q

Define a compound [1]

A
  • Made of more than one type of atom chemically bonded together
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3
Q

Define a mixture [2]

A
  • Two or more elements or compounds mixed together
  • Can be separated by physical means
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4
Q

Describe properties of metals [8]

A
  • Usually solids at room temperature
  • Malleable
  • Ductile
  • Shiny
  • High melting and boiling points
  • High density
  • High electrical conductivity
  • High thermal conductivity
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5
Q

What is the difference between a physical and a chemical change? [3]

A

Physical changes can involve;
- Change of state
- Separation of a mixture

Chemical changes involve;
- At least one new substance being made

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6
Q

What does ⇌ mean? [1]

A
  • Reversible reaction
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7
Q

What is the difference in colour between the anhydrous and hydrated forms of copper (II) sulphate? [2]

A
  • Anhydrous: white
  • Hydrated: blue
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8
Q

What is the difference in colour between the anhydrous and hydrated forms of cobalt (II) chloride? [2]

A
  • Anhydrous: blue
  • Hydrated: pink
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9
Q

Describe the structure of an atom [2]

A
  • Central nucleus containing protons and neutrons
  • Surrounding ‘shells’ of electrons
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10
Q

Describe the relative mass and charge of following; protons, neutrons and electrons [6]

A

Protons:
- 1
- (+1)

Neutrons:
- 1
- (+-0)

Electrons
- 0 (1 over 2000)
- (-0)

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11
Q

Describe the configuration of the inner three shells of an electron [4]

A
  • Innermost shell: 2 electrons
  • Second shell: 8 electrons
  • Third shell: 8 electrons
  • Total: 18 electrons
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12
Q

Why are the elements in group 0 (the noble gases) unreactive? [1]

A
  • Because they have full outer shells of electrons
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13
Q

How is group number on the periodic table related to electronic structure? [1]

A
  • Group number = number of valance electrons
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14
Q

How is period number on the periodic table related to electronic structure? [1]

A
  • Period number = number of occupied electron shells
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15
Q

What is the atomic number of an element? [1]

A
  • The number of protons in an atom
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16
Q

What is the mass number of an element? [1]

A
  • The number of nucleons (protons + neutrons) in an atom
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17
Q

How are the elements arranged in the periodic table? [2]

A
  • In ascending atomic number
  • Elements with similar properties arranged in groups
18
Q

Define isotope [2]

A
  • An atom of the same element but with a different number of neutrons
    + Changes atomic mass
19
Q

Why do isotopes have the same chemical properties? [1]

A
  • Because they have the same number of valance electrons
20
Q

Describe how metal atoms form ions [1]

A
  • Metals lose electrons to form positive ions
21
Q

Describe how non-metal atoms form ions [1]

A
  • Non-metals gain electrons to form negative ions
22
Q

Describe an ionic bond [1]

A
  • The electrostatic force of attraction between positive metal ions and negative non-metal ions
23
Q

What type of structure does ionic substances form? [1]

A
  • Giant ionic lattice
24
Q

Describe the properties of ionic substances [4]

A
  • Low volatility
  • High solubility
  • High melting and boiling point
  • Conducts electricity when molten or aqueous
25
Q

Do ionic substances have high or low melting and boiling points? Explain [3]

A
  • High
  • Strong electrostatic force of attraction between ions that…
    + …requires a lot of energy to overcome
26
Q

Do ionic substances conduct electricity? Explain [2]

A
  • Only when molten or aqueous
    + Because the ions are free to move and carry charge
27
Q

Describe a covalent bond [1]

A
  • A shared pair of electrons between non-metal atoms
28
Q

Describe the properties of covalent substances [4]

A
  • High volatility
  • Low solubility
  • Low melting and boiling point
  • Does not conduct electricity
29
Q

Do covalent substances have low or high melting and boiling points? Explain [3]

A
  • Low
  • Weak intermolecular forces of attraction that…
    + …require a small amount of energy to break
30
Q

Do covalent substances conduct electricity? Explain [2]

A
  • No
  • No free mobile charge carriers (electrons or ions) to carry charge through the structure
31
Q

Name three covalent macromolecules [3]

A
  • Diamond
  • Graphite
  • Silicon (IV) oxide
32
Q

Describe the structure and properties of diamond [8]

A
  • Giant covalent structure
    + lots of covalent bonds
  • Made of carbon
    + Each carbon atom bonds with four other carbon
    atoms
  • High melting point
    + Because of lots of covalent bonds that require a lot of
    energy to break
  • Does not conduct electricity
    + Because it doesn’t have any mobile charge carriers
33
Q

Describe the structure and properties of graphite [8]

A
  • Giant covalent structure
    + Lots of covalent bonds in layers (layered structure)
    + Weak intermolecular forces of attraction between
    layers
  • Conducts electricity
    + C atoms form 3 covalent bonds with other carbon
    atoms so it has one delocalised electron (mobile
    charge carrier)
  • High melting point
    + because of lots of covalent bonds that require a lot of
    energy to break
  • Still is a giant structure despite intermolecular forces
34
Q

Describe the structure of silicon (IV) oxide [2]

A
  • Giant covalent structure
  • One silicon atom for every two oxygen atoms
35
Q

Do these macromolecules have high or low boiling and melting points? [3]

A
  • High
  • Lots of strong covalent bonds that…
    + …require a lot of energy to break
36
Q

Is graphite able to conduct electricity? Explain [3]

A
  • Yes
  • C atoms form 3 covalent bonds so it has one
    delocalised valance electron (mobile charge carrier)
    + The mobile charge carrier can carry charge through the structure
37
Q

Explain why graphite is slippery [1]

A
  • The layers have weak intermolecular forces so the layers can slide off each other
38
Q

How is graphite used? [2]

A
  • As a lubricant
  • As a conductor
39
Q

How is diamond used? [1]

A
  • In cutting tools
40
Q

Define cation [1]

A
  • Positively charged ion
41
Q

Define anion [1]

A
  • Negatively charged ion

Chemistry (7 decks)

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