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additional chemistry > topic 1 > Flashcards

topic 1 Flashcards

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1
Q

how many electrons are In the

1st, 2nd, 3rd and 4th shell?

A

2,8,8,8

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2
Q

what is the nucleus made up of?

A

protons and neutrons

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3
Q

where is the nucleus?

A

middle of an atom

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4
Q

what overall charge does a nucleus have?

A

positive

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5
Q

is the nucleus tiny or big compared to the rest of the atom?

A

tiny

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6
Q

what do electrons do?

A

move around the nucleus

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7
Q

what charge do electrons have?

A

negative

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8
Q

are electrons tiny or big compared to the nucleus?

A

tiny

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9
Q

are the number of protons and electrons equal?

A

yes

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10
Q

the number of neutrons is usually…

A

about the same as the number of protons

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11
Q

are protons heavy/light and positive/negative charge

A

heavy and positive

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12
Q

neutrons are heavy/light and positive/negative/neutrally

A

heavy and neutral

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13
Q

are electrons tiny/heavy and negative/positive

A

tiny and negative

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14
Q

what electron shells are filled first?

A

the ones closest to the nucleus

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15
Q

why do atoms want full outer shells?

A

they are happier - more stable

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16
Q

why do most atoms want to react?

A

they don’t have a full outer shell

17
Q

elements consist of how many atoms?

A

only one

18
Q

each element has a different number of …

A

protons

19
Q

how do you determine what element it is?

A

the number of protons

20
Q

what is an atomic number?

A

the amount of protons in an atom - so same as the number of electrons

21
Q

what is the mass number?

A

amount of protons and neutrons in an atom

22
Q

how do you work out the amount of neutrons?

A

atomic number - mass number

23
Q

what are isotopes?

A

isotopes are different atomic forms of the same element which have the same number of protons but different number of neutrons

24
Q

give an example of an isotope

A

Carbon - 12 and carbon 14

25
Q

how do you work it the relative atomic mass?

A

1) multiply the mass of each isotopes but it’s relative abundance (fraction,percentage,ratio)
2) add those together
3) divide by the sum of the relative abundance

26
Q

in the old period ice table what order where the elements put in?

A

in order of their atomic number

27
Q

who arranged the periodic table?

A

dmitri mendeleev

28
Q

what did dmitri mendeleev arrange the emergents into?

A

groups

29
Q

mendeleev arranged elements according to there what?

A

properties

30
Q

what are similarities of the old and new periodic table?

A

the elements are arranged noticing similar chemicals and physical properties
both are organised by groups

31
Q

what are differences of the old and new periodic table?

A

mendeleevs table included 63 elements but the modern one consists of 109 elements
mendeleevs table was based on atomic mass and the periodic table is organised by atomic number
Mendeleev predicted where several undiscovered elements would fall in the table and left room for them

32
Q

what is ionic bonding?

A

the transfer of electrons

33
Q

what happens when an atom transfers (loses) an electron? (ionic bonding)

A

forms a positive atom called an cation

34
Q

why do alkali metals react with halogens? (ionic bonding)

A

because alkali metals only have on e electron in their outer shell so they are keen to get rid or gain an electron as they want a full outer shell.

35
Q

does an atom become a positive or negative ion if they lose an electron?

A

positive (cation)

36
Q

do metals lose or gain electrons?

A

loose

37
Q

do non-metals loose or gain electrons?

A

gain

38
Q

what are the most likely groups to form ionic bonds?

A

1&2 and 6&7

39
Q

what is the structure of an atom?

A

nucleus

electron shells

additional chemistry (6 decks)

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