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year 9 > Chemistry > Flashcards

Chemistry Flashcards

1
Q

what is an atom?

A

building blocks of all materials everything is made up of atoms.

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2
Q

what is an element?

A

substrate made up if one kind of atom.

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3
Q

what do atoms combine to form?

A

compounds

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4
Q

how to find the number of elements?

A

count the capital letters

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5
Q

what are the reactants?

A

react together to form products. they are found on the left side of the equation.

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6
Q

what is a mixture?

A

consists of two or more elements or compounds that are not chemically bonded together.

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7
Q

how can mixtures be separated?

A

by physical processes. they don’t involve chemical reactions and no new substances are made.

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8
Q

what is magnetism?

A

separates magnetic material from non- magnetic material.

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9
Q

what is evaporation?

A

separates a soluble solid by burning off.

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10
Q

what is filtration?

A

separates an insoluble solid from a liquid.

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11
Q

what is distillation?

A

separates liquids with different boiling points.

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12
Q

what is chromatography?

A

separates liquids of different colours.

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13
Q

what is crystallisation?

A

the forming of crystals in a liquid.

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14
Q

what was Dalton’s representation of the atom?

A

suggested that atoms were tiny spheres that could not be divided.

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15
Q

what was JJ Thomson’s representation of the atom?

A

discovered the electron. he suggested the plum pudding model. ball of positive charge with negative electrons.

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16
Q

what came after the plum pudding?

A

the atoms had loads of particles fired at them. this gave the scientists the idea of the nucleus as some particles passes through but not all.

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17
Q

what was Ruthford’s representation of the atom?

A

created an alpha particle scattering experiment. nuclear model of the atom suggested.

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18
Q

what was Neil Bohr’s representation of the atom?

A

adapted the model to suggest that atoms orbit the nucleus at specific distances.

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19
Q

what was James Chadwick’s representation of the atom?

A

went on to prove the existence of neutrons.

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20
Q

what is relative atomic mass?

A

protons and neutrons added together.

21
Q

what is the atomic number?

A

the protons are the same number as the electrons.

22
Q

how are the elements in the periodic table arranged?

A

by atomic number

23
Q

what does the periodic table tell you?

A

how many number of shells an atom has.

24
Q

what was Mendeleev’s idea?

A

changed order of some elements when arranged by atomic weight. then he changed it but left gaps for undiscovered atoms. it was incomplete but he ended up getting the properties he predicted.

25
Q

what are group 0 atoms?

A
  • called the noble gasses
  • as you go down the group the boiling point increases. this because of the size of the molecules gets larger so the strength of the intermolecular forces increases.
  • more energy needed to break the bonds.
  • they have 8 electrons in their outer shell.
  • unreactive and do not easily form molecules because their atoms have stable arrangements of electrons.
26
Q

what are group 1 atoms?

A
  • known as the alkali metals
  • as you go down the group, they become more reactive
  • outermost electrons are further away from the nucleus
  • outermost electrons are more easily lost.
27
Q

what are group 7 atoms?

A
  • known as halogens
  • melting& boiling point increase down the group

-7 electrons in outer shell

  • a more reactive halogen will also replace a less reactive halogen from solutions of its salt.
28
Q

what is ionic bonding?

A

bonding between non- metals and metals where electrons are shared.

29
Q

what is metallic bonding?

A

bonding between two or more metals where the electrons are given or taken.

30
Q

what is covalent bonding?

A

bonding between two or more non- metals where electrons are shared.

31
Q

what is it called when you move from a gas to a solid?

A

deposition.

32
Q

what are the letter representations for states of matter?

A

solid(s)
liquid(l)
gas(g)
solution(eq)

33
Q

what are polymers?

A
  • covalent that bonded substrates and have very large molecules.
  • intermolecular forces between polymers are relatively string and so these substrates are solids at room temperature.
  • atoms are linked to other atoms by strong covalent bonds.
34
Q

what are metals surrounded in?

A

a sea of electrons.

35
Q

what are the properties of ionic compounds?

A
  • high melting and boiling points
  • can’t conduct electricity
  • can conduct when molten or dissolved.
36
Q

what is a high melting point?

A

lots of energy used to overcome the strong electrostatic bonds that are acting in all directions.

37
Q

what does it mean if something can’t conduct electricity?

A

when solid, the ions are vibrating in fixed positions. they are unable to move freely and so as a solid ionic compounds don’t conduct electricity.

38
Q

what does it mean if something can conduct electricity when molten or dissolves?

A

the solid ions are dissolves or molten, the ions are able to move freely and so able to conduct electricity.

39
Q

what are giant covalent structures?

A
  • giant covalent structures are solids with very high melting points.
  • all of the atoms are linked by strong covalent bonds.
  • must be overcome to melt or boil these substrates.
40
Q

what are properties of metals and alloys?

A
  • soft
  • high melting point
  • good conductors of electricity
  • easily bent and shaped.
  • good conductors of thermal energy.
41
Q

differences between alloys and metals

A

-alloys are harder than metals
- atoms are different sizes
- layers distorted
- layers unable to slid under each other.

42
Q

why are metals good conductors of electricity?

A

the delocalised electrons in the metal carry electrical charge through the metal.

43
Q

why are metals good conductors of thermal energy?

A

energy is transferred by the delocalised electrons.

44
Q

what are the properties of diamond?

A
  • high melting and boiling points.
  • doesn’t conduct electricity
  • each carbon atom forms four covalent bonds with other carbon atoms in a giant covalent structure.
45
Q

what are the properties of graphite?

A
  • each carbon atom forms three covalent bonds with other carbon atoms. they form layers of hexagonal rings which have no covalent bonds between the layers.
  • one electron from each carbon atom is delocalised
  • high melting and boiling point
  • soft
  • conducts electricity
46
Q

what are fullerenes?

A

molecules of carbon atoms with hollow shapes

47
Q

what is the structure of fullerenes based on?

A

hexagonal rings of carbon atoms but they may also contain rings with five or seven carbon atoms.

48
Q

what are carbon nano-tubes?

A

cylindrical fullerenes with very high length to diameter ratios.

49
Q

what would happen if the size of a cube decreases by a factor of 10?

A

the surface area to volume ratio would increase by a scale factor of 10.

year 9 (3 decks)

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