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gcse > chem nov 1st (C1, C2) > Flashcards

chem nov 1st (C1, C2) Flashcards

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1
Q

What is the main difference between a physical change and a chemical change?

A

In a physical change no new substances are made. In a chemical change at least one new substance is made.

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2
Q

What is the difference between a mixture and a compound?

A

In a compound the elements are chemically combined together. In a mixture the elements or components are not chemically combined together.

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3
Q

What can affect diffusion?

A

-temperature
-particle mass
-air particles/solvent particles can affect the rate

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4
Q

What are the arrangements of electrons called?

A

electron configuration

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5
Q

Metals are often malleable. What does this mean?

A

A malleable substance can be beaten or hammered into shape.

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6
Q

What are some typical properties of metals?

A

good conductors of electricity and heat, shiny, malleable, ductile, sonorous, high melting points

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7
Q

How are electrons arranged

A

in shells

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8
Q

how many electrons can the first shell hold

A

2

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9
Q

How many electrons can the second and further shells hold?

A

maximum of 8

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10
Q

What are some typical properties of non-metals?

A

poor conductors of electricity and heat, dull, brittle, low melting points

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11
Q

Sodium has 11 electrons, what is the electron configuration?

A

2,8,1

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12
Q

Which sub-atomic particle has the smallest relative mass?

A

Electron

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13
Q

what are the electrons in the outer shells that are involved in chemical bonding known as?

A

valency electrons.

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14
Q

Why do atoms have the same number of protons as electrons?

A

Atoms are neutral. The number of positive charges (protons) must equal the number of negative charges (electrons).

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15
Q

What are isotopes?

A

Isotopes are atoms of the same element with different numbers of neutrons.

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16
Q

why are helium, neon, argon and krypton so unreactive?

A

they all have 8 electrons in their outer shells or full outer shells

this means the atoms don’t lose or gain electrons easily.

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17
Q

what is formed when one of the reacting atoms is a metal and the other is a non metal?

A

an ionic compound. it is made up of ions.

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18
Q

what is an example of an isotope

A

Chlorine exists as two different chlorine atoms.

  1. chlorine 35 (17 protons 18 neutrons)
  2. chlorine 37 (17 protons 20 neutrons)
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19
Q

Why do isotopes of the same element have the same chemical properties?

A

as they have the same number of electrons in the outer shell which determines its chemical behaviour

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20
Q

Why are noble gases unreactive?

A

The noble gases have full outer shells, they do not easily lose or gain electrons.

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21
Q

Why are noble gases stable?

A

because they have full outer shells.

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22
Q

Why does a covalently bonded compound such as carbon dioxide have a relatively low melting point?

A

The intermolecular forces of attraction between the molecules are weak.

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23
Q

What will electron arrangements always match

A

A noble gas’s electron configuration (full outer shell)

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24
Q

What does carbon not form

A

ions

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25
Q

Would you expect a covalently bonded compound such as ethanol to conduct electricity? Explain your answer.

A

No. There are no ions or delocalized electrons present.

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26
Q

What are cations

A

positively charged ions

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27
Q

What are anions

A

negatively charged ions

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28
Q

Explain why a diamond has a very high melting point.

A

Each carbon atom is strongly covalently bonded to four other atoms forming a very strong giant lattice structure. A very high temperature is needed to break down the structure.

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29
Q

What is ionic bonding

A

The electrostatic attraction between oppositely charged ions

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30
Q

How is the structure of a graphite different from that of diamond?

A

Graphite, on the other hand, has a layered structure with each carbon atom forming strong covalent bonds with three other carbon atoms within each layer. Weak intermolecular forces hold these layers together.

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31
Q

What does electrostatic mean

A

stationary or slow-moving electric charges.

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32
Q

What patterns are ions in an ionic compound arranged into?

A

an ionic lattice

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33
Q

oxidation

A

metals lose electrons

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34
Q

reduction

A

non metals gain electrons

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35
Q

what are ions

A

atoms or groups of atoms that have gained or lost electrons

36
Q

When an atom gains an electron how is that written in a diagram

A

(if it loses more than one it is written in front of the sign) - (minus)

36
Q

What is ionic bonding between

A

metals and non metals

37
Q

Describe how the arrangement of particles changes during melting.

A

the arrangement of the particles changes from orderly and tightly packed, to randomly arranged and tightly packed.

38
Q

What do ionic substances consist of

A

non metals and metals

39
Q

Describe how the arrangement of particles changes during evaporation.

A

During evaporation the arrangement of the particles changes from randomly arranged and tightly packed, to randomly arranged and spread apart.

40
Q

Describe how the movement of particles changes during melting.

A

During melting, a solid becomes a liquid. In a solid, the particles vibrate on the spot, in a liquid they flow over each other

41
Q

Describe how the movement of particles changes during evaporation.

A

During evaporation, liquid turns into gas. In a liquid, the particles flow over each other and interact, whereas in a gas the particles move around freely.

42
Q

what subatomic particles stay the same in all atoms

A

protons

43
Q

Describe the arrangement of particles in gas.

A

The particles are spaced far apart and in a random arrangement.

44
Q

what are covalent bonds

A

a pair of electrons shared by atoms

45
Q

Describe the arrangement of particles in liquid.

A

The particles are packed tightly together and have a random arrangement.

46
Q

Describe the arrangement of particles in solid.

A

The particles must be packed tightly together and must all be touching in a uniform structure.

47
Q

Describe the movement of particles in a solid

A

vibrate on the spot

48
Q

Describe the movement of particles in a liquid

A

the particles can move over each other

49
Q

whats an example of covalent molecules

A

Water (H₂O)
Carbon dioxide (CO₂)
Methane (CH₄)
Ammonia (NH₃)
Hydrogen chloride (HCl)

50
Q

Describe the movement of particles in a gas

A

particles can move freely and are constantly moving in random directions

51
Q

whats an example of giant covalent lattices

A

diamonds, graphite, silicon dioxide

52
Q

polyatomic ions

A

Hydroxide OH⁻ -1
Carbonate CO₃²⁻ -2
Sulfate SO₄²⁻ -2
Nitrate NO₃⁻ -1
Hydrogen Carbonate HCO₃⁻ -1
Phosphate PO₄³⁻ -3
Ammonium NH₄⁺ +1

53
Q

Explain why graphite has a high melting point.

A
  • graphite is a giant covalent lattice
  • many strong covalent bonds require lots of energy to overcome
54
Q

Explain why diamond has a very high melting point.

A
  • diamond is a giant covalent lattice
  • it has a tetrahedral structure where each carbon is bonded to 4 other carbon
  • need to break many covalent bonds which require lots of energy to break
55
Q

What is an element?

A

a substance containing only one type of atom

56
Q

What is a compound?

A

a substance containing two or more types of atoms chemically joined together

57
Q

What is a mixture?

A

a mixture can contain elements and compounds but the substances are not chemically joined

58
Q

What is nuclide notation?

A

nuclide notation shows the element symbol, proton (atomic number), and nucleon (relative atomic mass).

59
Q

When will ionic compounds conduct electricity?

A

will conduct electricity in solution or molten, not when solid

60
Q

What is a diatomic molecule?

A

a molecule made of only two atoms bonded together

61
Q

What is a triatomic molecule?

A

a molecule made of only three atoms bonded together

62
Q

What is valency?

A

the number of bonds an element needs to form

63
Q

what are some properties of ionic compounds

A

High Melting and Boiling Points: Strong electrostatic forces between ions require a lot of energy to break.

Hardness and Brittleness: The rigid lattice structure makes them hard but brittle.

Solubility: Many are soluble in water, forming aqueous solutions.

Reactivity: Can react with other substances to form new compounds.

64
Q

What are intramolecular bonds?

A

the forces that hold atoms together within a molecule

65
Q

What are intermolecular forces?

A

the forces that exist between molecules, intermolecular forces are weaker than intramolecular bonds

66
Q

What happens when a molecular substance is melted or boiled?

A

the strong bonds between atoms are not broken, the weaker forces of attraction between molecules are broken

67
Q

Why does an ionic compound such as magnesium oxide not conduct electricity when it is solid?

A

The ions are held together strongly in a giant lattice structure. The ions can vibrate but not move around

68
Q

what are ions in an ionic compound arranged into

A

ionic lattices

69
Q

How does electrical conductivity change in ionic compounds

A

Ionic compounds will not conduct electricity when solid but will in solutions or molten.

70
Q

are ionic compounds intermolecular forces strong or weak

A

strong

71
Q

are simple covalent compounds intermolecular forces strong or weak

A

weak

72
Q

Why do ionic compounds only conduct electricity when dissolved in a solvent?

A

When an ionic substance is dissolved in solution (or molten) the ionic lattice is is broken down allowing the ions to move freely. This allows conduction to occur.

73
Q

structure of ionic compounds

A

Ionic compounds have a giant ionic lattice structure. This means they form a 3D structure with alternating positive and negative ions. The strong electrostatic attraction between these oppositely charged ions holds the structure together.

74
Q

what are the intermolecular forces between the covalent molecule like

A

While the atoms within a covalent molecule are held together by strong covalent bonds, the forces between different molecules are much weaker.

75
Q

characteristics of covalent molecular substances

A

Low melting points
low boiling points

76
Q

what does volatile mean

A

evaporate easily

77
Q

why do covalent molecules have low boiling and melting points

A

covalent molecules do not require as much energy to break bonds as the intermolecular forces are much weaker

78
Q

properties of metals

A

strong, malleable, ductile, hard, high melting points & boiling points, sonorous, high tensile strength (maximum strength a material can be stretched with)

79
Q

Why are metals good conductors of heat and electricity?

A

delocalised electrons which can move freely throughout the metal lattice, allowing for the easy transfer of heat energy and electric charge.

80
Q

what is the definition of metallic bonding

A

It is the electrostatic attraction between positively charged metal cations and a sea of delocalised electrons.

81
Q

Why are metallic compounds malleable and ductile

A

cations are organised in to layers which can slide over eachother.

82
Q

What do imfs only apply to

A

covalent molecules

83
Q

How do you differentiate between metallic, covalent or ionic bonds

A

Ionic bonds involve the transfer of electrons between atoms, forming oppositely charged ions that attract each other.

Covalent bonds involve the sharing of electron pairs between atoms.

Metallic bonds involve a lattice of metal ions surrounded by a ‘sea’ of delocalised electrons, allowing for high conductivity.

84
Q

How are metallic compounds structured (draw it)

A

+ - + - + - + - + - = delocalised electrons
+ - + - + - + - + + = metal cations
+ - + - + - + - +

gcse (2 decks)

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