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atomic structure and the periodic table Flashcards

1
Q

what is a pure substance

A

consists of only one element or compound

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2
Q

who published the first ideas about atoms in 1803

A

John Dalton, tiny spheres that couldn’t be divided

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3
Q

who discovered the electron

A

JJ Thompson, led him to suggesting the plum pudding model of the atom, ball of positive charge with negative electrons embedded

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4
Q

who did the gold foil experiment in 1909

A

Ernest Rutherford

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5
Q

what conclusions did he make from the gold foil experiment

A

most passing straight through - mostly empty space
change direction - positive centre
reflecting - mass of atom concentrated in centre

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6
Q

who proved that electrons orbited in shells

A

Niels Bohr

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7
Q

who discovered neutrons in 1932

A

James Chadwick

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8
Q

what proportion of a nucleus is the atom

A

1/10.000

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9
Q

do isotopes of the same element have identical chemical properties

A

yes

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10
Q

when did mendeleev publish his first periodic table

A

1869

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11
Q

how did mendeleev arrange the first periodic table

A
  • in order of increasing weight taking into account properties of elements and compounds
  • this meant his table had gaps
  • elements with similar properties lined up in groups
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12
Q

what happened as a result of mendeleev leaving gaps

A

he predicted properties of future elements that turned out to be true

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13
Q

what is an explanation for mendeleev pair resversals

A

different isotopes of elements existed, elements with higher relative atomic mass had lower atomic numbers

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14
Q

do metals lose or gain electrons

A

lose electrons

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15
Q

what is the difference between metal and non-metal oxides

A

metal oxides are basic

non-metal oxides are acidic

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16
Q

what does malleable mean

A

means it can be hammered into shape without breaking

17
Q

what does ductile mean

A

means it can be made into a wire

18
Q

what is group 0

A

noble gases - on the far right of the periodic table

19
Q

why do noble gases increase in boiling points

A
  • atoms become larger
  • intermolecular forces between atoms are stronger
  • more energy needed to overcome these forces
20
Q

what does inert mean for noble gases

A

extremely unreactive

21
Q

why are noble gases unreactive

A

they already have a full outer shell so don’t need to lose gain or share electrons

22
Q

what is group 1

A

alkali metals - on the far left of the periodic table

23
Q

physical properties of alkali metals

A
  • soft
  • low melting points
  • low densities
24
Q

what happens to melting points for alkali metals

A

decrease

25
Q

what happens when alkali metals react with water

A

produce a metal hydroxide + hydrogen

26
Q

what do alkali metals melt to form in water

A

a ball

27
Q

what happens when alkali metals react with oxygen

A

produce metal oxides as white smoke

28
Q

what happens when alkali metals react with chlorine

A

form white solid chlorides that dissolve in water to form colourless solution

29
Q

why do alkali metals get more reactive

A
  • atoms become larger
  • outer electron further from nucleus
  • force of attraction between nucleus and outer electron decreases
  • outer electron lost more easily
30
Q

what is group 7

A

halogens on the second to right hand side of periodic table

31
Q

how do halogens exist

A

a pair of halogen atoms joined by a single covalent bond

32
Q

what happens to melting and boiling points in halogens

A

increase as you go down because

  • molecules become larger
  • intermolecular forces become stronger
  • more energy needed to overcome these forces
33
Q

what happens when a halogen reacts with metals

A

produces salts held together by ionic bonds

34
Q

what happens to reactivity as you go down halogens

A

decreases

35
Q

what happens when a halogen reacts with hydrogen

A

hydrogen halide is formed gas at room temperature which dissolve in water to produce acidic solutions

36
Q

reactivity series

A 
potassium
sodium 
calcium
magnesium
aluminium
carbon
zinc
iron
tin
lead
hydrogen
copper
silver
gold 
platinum
37
Q

properties unique to transition metals

A
  • higher melting points
  • higher densities
  • greater strength
  • greater hardness
38
Q

what coloured compounds do the different metals form

A

not transition - white compounds

transition - coloured compounds

39
Q

what is a catalyst

A

substance that increases rate of reaction without being used up

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