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Chemistry - Paper 1 > ATOMIC STRUCTURE & PERIODIC TABLE > Flashcards

ATOMIC STRUCTURE & PERIODIC TABLE Flashcards

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1
Q

what is an atom

A

smallest part of an element that can exist

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2
Q

what is Daltons model of the atom

A

atoms are solid spheres that could not be divided into smaller parts

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3
Q

what is the plum pudding model of the atom

A

sphere of positive charge with negative electrons embedded in it

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4
Q

what did scientists discover in the alpha scattering experiment

A

some alpha particles were deflected by the gold foil, this showed that an atoms mass and positive charge must be concentrated in one small space

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5
Q

describe the nuclear model of the atom

A

dense nucleus with electrons orbiting it

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6
Q

what did James Chadwick discover

A

uncharged particles particle called a neutron

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7
Q

where are protons and neutrons

A

nucleus

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8
Q

how can you find the number of protons in an atom

A

the atomic number on the periodic table

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9
Q

how can you calculate the number o neutrons in an atom

A

mass number - atomic number

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10
Q

why do atoms have no overall charge

A

equal numbers of positive protons and negative electrons

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11
Q

what is an element

A

substance made of one type of atom

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12
Q

what is a compound

A

substance made of more than one type of atom chemically joined together

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13
Q

what is a mixture

A

2 or more substances not chemically combined

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14
Q

what is an isotope

A

atom of the same element - dame number of protons but different number of neutrons

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15
Q

4 physical processes to separate mixture

A

filtration, crystallisation, fractional distillation and chromatography

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16
Q

what is relative mass

A

the average mass of all the atoms in an element

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17
Q

how is the modern periodic table ordered

A

atomic number

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18
Q

how were the early lists of elements ordered

A

atomic mass

19
Q

why did Mendeleev swap the order of some elements

A

to group them by their chemical properties

20
Q

why did Mendeleev leave gaps in his periodic table

A

leave room for elements that had not yet been discovered

21
Q

why do elements in a group have similar chemical properties

A

have same number of electrons in their outer shell

22
Q

what is name given to group 1 metals

A

alkali metals

23
Q

why are the alkali metals named this

A

they are metals that react with water to form an alkali

24
Q

give the general equations for the reactions of alkali metals with oxygen, chlorine and water

A

metal + oxygen —-> metal oxide
metal + chlorine —> metal chloride
metal + water —> metal hydroxide + hydrogen

25
Q

how does the reactivity of the alkali metals increase down the group

A

increases because they are larger atoms so the outermost electron is further from the nucleus, meaning there are weaker electrostatic forces of attraction and more shielding between the nucleus and outer electron, and its easier to lose the electron

26
Q

what is the name given to group 7 elements

A

halogens

27
Q

how do the melting points of halogens change down the group

A

increase

28
Q

how does the reactivity of the halogens change down the group

A

decrease because they are larger atoms so the outermost electron is further from the nucleus meaning there are less electrostatic forces of attraction and more shielding between the nucleus and outer shell so its harder to gain an electron

29
Q

what is a displacement reaction

A

when a more reactive element takes the place of a less reactive one in a compound

30
Q

what is the name given to group 0 elements

A

noble gases

31
Q

why are noble gases inert

A

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

32
Q

how do the melting points of noble gases change down the group

A

increase

33
Q

how do the melting points of transition metals compare to those of group 1 metals

A

higher

34
Q

how do the densities of transition metals compare to those of group 1 metals

A

higher

35
Q

how do the strengths of transition metals compare to those of group 1 metals

A

higher

36
Q

how does the hardness of transition metals compare to those of group 1 metals

A

higher

37
Q

how does the reactivity of transition metals with oxygen, halogens and water compare to those of group 1 metals

A

lower

38
Q

what are transition metals used for

A

catalysts

39
Q

give the distinctive properties of transition metals

A

form ions with different charges and coloured compounds

40
Q

how big are nanoparticles

A

1-100 nm

41
Q

how are nano materials different from bulk materials

A

nano materials have a much higher surface area to volume ratio

42
Q

what are nanoparticles used for

A

healthcare, electronics, cosmetics and catalysts

43
Q

how big are fine particles

A

100-2500 nm

Chemistry - Paper 1 (5 decks)

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