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chemistry one > atomic structure and the periodic table > Flashcards

atomic structure and the periodic table Flashcards

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1
Q

what are atoms made out of

A

smaller particles and has the basic structure of a nucleus containing neutrons and protons and surrounding shells containing electrons

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2
Q

what is the relative mass of protons, neutrons and electrons

A

protons and neutrons = relative mass of 1
electrons = very very small sometimes referred to as 0

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3
Q

what is the charge of protons, neutrons and electrons

A

protons = positive +1
neutrons = natural no charge
electrons = negative -1

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4
Q

what is the radius of an atom

A

0.1 nm

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5
Q

what is an ion

A

when the charges of protons and electrons are equal the atom is neutral, yet when the charges are not balanced, the atom is then called an ion (either positive or negative)

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6
Q

what is an element

A

different types of atoms

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7
Q

what is the number in the bottom left representative of

A

atomic number and represents the number of protons. this determines the element it is

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8
Q

what is the number in the top right representative of

A

mass number

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9
Q

what is an isotope

A

different forms of the same element that have the same number of protons but have a different number of neutrons

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10
Q

what is relative atomic mass

A

the average mass of all the isotopes that make up an element

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11
Q

what is abundance

A

how common/rare a specific isotope is

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12
Q

how do you work out the relative atomic mass

A

sum of (isotope abundance x isotope mass)
————————————————————
sum of abundances of all the isotopes

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13
Q

work out the relative mass of copper
where copper - 63 = 69.2%
and copper - 65 = 30.8%

A

69.2 x 63 + 30.8 x 65 = 6361.9

69.2 + 30.8 = 100

= 63.6169

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14
Q

what is a molecule

A

2 or more atoms held together by a chemical bond for example oxygen, water and chlorine

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15
Q

what is a compound

A

2 or more different elements held together by a chemical bond for example water, carbon dioxide. they are always found in the same proportion for example water = h2o

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16
Q

what is a mixture

A

containing two or more substances that are not chemically combined together (they haven’t reacted). these are easily separated

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17
Q

who was Democritus

A

he created the first theory of the atom
- atomic theory
the idea that everything is made up of tiny particles and are separated by empty space

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18
Q

who was John Dalton

A
  • solid spheres
    the idea that different shaped/sized atoms where different elements
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19
Q

who created the plum pudding model

A

J J Thomson

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20
Q

explain the Plum pudding model

A

the idea that the atoms couldn’t be spheres and Thomson believed atoms were spread out balls of positive charge with discreate electrons in it

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21
Q

who was Earnest Rutherford

A

he proved the plum pudding model to be wrong

he then created the Nuclear model
- the idea that their was a compact nucleus with a positive charge with negative charge surrounding it

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22
Q

who is Neil Bohr

A

suggested electrons orbit nucleus and are held in shells

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23
Q

what did Rutherford and James Chadwick discover to add to Neil Bohr’s findings

A

Rutherford - found protons in nucleus
Chadwick - found neutrons in nucleus

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24
Q

how is an atom stable

A

needs a full outer shell

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25
Q

how does an atom become stable

A

the atom needs to react with another atom to gain or loose the electron they need

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26
Q

which shell has the lowest energy level

A

closest to the nucleus

27
Q

which group on the periodic table have all their atoms with a full outer shell

A

the noble gasses - group 0

28
Q

how do you draw an electron structure for an atom use argon as an example. this has an atomic number of 18

A

first shell - 2 electrons
second shell - 8 electrons
third shell - 8 electrons

29
Q

how does the atom calcium become an ion

atomic number of 20

A

first shell - 2
second shell - 8
third shell - 8
fourth shell - 2

the atom looses two electrons in order to have a full outer shell
this atom is then written in brackets with the two lost electrons. outside the bracket write 2+

30
Q

if the atom is gaining an electron in order to become stable how is the brackets written out

A

in brackets yet outside write -x
when x is how many electrons are gained

31
Q

how are elements arranged

A

increasing atomic number moving from left to right

32
Q

explain what information is stated in each box in the periodic table

A

elemental sign, atomic number (electrons), mass number (protons and neutrons)

33
Q

what is a period

A

a specific group of elements that share similar chemical properties

34
Q

explain what elements in the same group have in common

A
  • the same number of electrons in their outermost shell. The group number tells you how many electrons are in the outer most shell
35
Q

what did Dobereiner find out

A

he realised that elements with similar properties often occurred in threes

36
Q

what law did Newland create

A

law of octave
- arranged the elements in order of atomic weight, he also stated that every 8th element reacts in a similar way
- because of this, elements were grouped together even if they have different properties

37
Q

who created the modern periodic table

A

Dmitri Mendeleev

38
Q

explain how Dmitri Mendeleev created the modern day periodic table

A
  • started by arranging all the elements in order of increasing atomic weight
  • left gaps for future discovery of elements.
39
Q

what are some differences between the modern day periodic table and Mendeleev’s periodic table

A

modern day - in order of atomic number (protons)
Mendeleev - protons weren’t discovered and therefore elements were in order of atomic weight. this caused some elements to appear wrong due to isotopes

modern day - has noble gasses
Mendeleev - not been discovered when he created it

40
Q

how did Mendeleev predict the properties of elements that hadn’t been discovered

A

he based his ideas on other elements in the same group.

41
Q

what type of ions do metal and non metal form when they react

A

metals - positive ions
non metals - negative ions OR don’t form ions

42
Q

why are metals more reactive as you move down a group

A

because the outermost shell is further from the nucleus, the positive nucleus can’t hold onto electrons in these shells. therefore they are able to get lost more easily.

43
Q

what are the physical properties of metals

A
  • metallic bonding
  • malleable
  • conductors of heat and electricity
  • high melting and boiling point
44
Q

what are the physical properties of non metals

A
  • brittle
  • low boiling point
  • poor conductors
  • lower density
45
Q

what are the properties of transition metals

A
  • form more than one ion
  • good catalysts
46
Q

what are the group one metals called

A

alkali metals

47
Q

what are the properties of alkali metals

A

the opposite of “normal metal”
- soft, low density, low melting point
- a lot more reactive

48
Q

as you go down the alkali metals group, what are the properties

A
  • more reactive (calcium ignite at room temperature)
  • melting and boiling point decreases
49
Q

what do alkali metals need to do to be stable and why are does the reactivity increase as you go down the group

A

loose one electron. as you go down the group, the outer shells gets further away from the nucleus as there is an increased weakness in attractive forces

50
Q

what happens when an alkaline metal reacts with water

A

alkali metals + h20 reacts vigorously to form metal hydroxide + hydrogen gas

reactions will release more energy as move down the group, elements near the end of the table could react with the hydrogen gas formed

51
Q

what happens when an alkaline metal reacts with chlorine gas

A

when metal is heated in chlorine gas it forms a white metal chloride salt. again reacting more vigorously when moving down the group

52
Q

what happens when an alkali metal reacts with oxygen

A

forms a metal oxide

53
Q

what happens when oxygen reacts with lithium

A

lithium oxide is formed

54
Q

what happens when oxygen reacts with soduim

A

sodium oxide OR sodium peroxide is formed

55
Q

what happens when oxygen reacts with potassium

A

potassium peroxide OR potassium superoxide

56
Q

what is group seven called

A

halogens

57
Q

explain what the properties of each element is
- Florine
- chlorine
- bromine
- iodine

A

fluorine - poisonous yellow gas, very reactive
chlorine - less reactive, poisonous green gas
bromine - red/brown poisonous liquid
iodine - dark grey solid which can form poisonous purple vapour (can be used as an antiseptic)

58
Q

what is a diatomic molecules

A

2 atom molecules - covalent bonds

59
Q

as you go down the halogen group what are the trends

A
  • melting and boiling point increases
  • reactivity decreases
60
Q

why does the reactivity decrease as you go down the group

A

the outer shell gets further away from the nucleus. attractive forces, which are needed to pull extra electrons for the atom, gets weaker. if a halogen can’t attract an electron to complete outer shell then it can’t react

61
Q

explain the ionic bonding halogens experience with metals

A

when reacting with metals ( most likely alkali metals) it becomes a negative ion - becoming a halide
( fluoride, chloride, bromide, iodide)

62
Q

what is the displacement theory

A

involves a more reactive halogen displacing a less reactive one

63
Q

explain the properties of group zero

A

noble gasses
- all exist as colourless gasses
- all have full outer shells and therefore don’t react with anything
- non flammable
- boiling point increases as you go down the group

chemistry one (8 decks)

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