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GCSE Chemistry > C1 Atomic structure and periodic table > Flashcards

C1 Atomic structure and periodic table Flashcards

1
Q

define element

A

made up of the same type of atom and cannot be chemically split up further

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2
Q

define compound

A

two or more different atoms that are chemically bonded

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3
Q

define mixture

A

two or more atoms that are not chemically bonded

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4
Q

define empirical formula

A

The simplest ratio of atoms of each element in a compound

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4
Q

define empirical formula

A

The simplest ratio of atoms of each element in a compound

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5
Q

how do you calculate the empirical formula?

A
  • count up number of each type of ion
  • divide by the smaller number
  • round to the nearest whole number
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6
Q

define solute

A

the name of what you dissolve

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7
Q

define solvent

A

the name of what you dissolve the solute in

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8
Q

define solution

A

the outcome of dissolving the solute in the solvent

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9
Q

define soluble

A

a name you give to a substance that can be dissolved

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10
Q

define insoluble

A

a name you give to a substance that cannot be dissolved

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11
Q

define solubility

A

the amount of solute that can be dissolved in 100g of solvent

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12
Q

through which experiment did John Thompson discover electrons mainly?

A

The Vaccum Tube

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13
Q

what did the experiment The Vacuum Tube show?

A

showed negatively charged particles flowing through an electrical current

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14
Q

what misconception did John Thompson think about electrons after the Vacuum Tube experiment?

A

he thought that electrons were part of the atom because they were much smaller and alike

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15
Q

what model of the atom did John Thompson make after the Vacuum Tube experiment?

A

the plum pudding model

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16
Q

describe the plum pudding model

A

had an area of positive space and had negative electrons randomly spotted in the middle

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17
Q

what experiment did Ernest Rutherford do?

A

the alpha particle scattering experiment

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18
Q

what was the alpha scattering experiment?

A

fired alpha particles (He2+ ions) at a piece of gold foil

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19
Q

what 4 things did Ernest Rutherford learn about the atom from the alpha particle scattering experiment?

A
  • there is a positive nucleus in the middle
  • electrons are around the nucleus
  • the mass of the atom is concentrated at the middle
  • most of the atom is space
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20
Q

how did Ernest know that there is a positive nucleus in the middle from the a.p.s experiment?

A

the particles were reflected/refracted by this and re-directed

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21
Q

how did Ernest know that the mass of the atom is concentrated in the middle from the a.p.s experiment?

A

some of the particles were deflected and some of them went straight through

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22
Q

describe what changes Bohr made to the nuclear model

A

he put electrons set distance from the nucleus and they are orbiting it, these are called shells/energy levels

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23
Q

describe 4 differences between the nuclear model and plum pudding model?

A

-plum pudding model has no nucleus
-in the ppm the mass was evenly distributed but in the nm its concentrated in the middle
-most of the nm is space but in the ppm there are no spaces
-in the ppm electrons are randomly plotted around but in the nm they are around the positive nucleus

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24
Q

why are lithium and sodium both in group 1?

A

they both have 1 electron in their outer shell

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25
Q

explain why sodium is more reactive than lithium

A

-sodium has more shells/its a bigger atom
-weaker force of attraction between outer electron and positive nucleus
-makes the outer electron easier to lose

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26
Q

give 2 observations you can see when potassium is added to water

A

-fizzing with bubbles
-the potassium floats on the water

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27
Q

explain why sodium oxide has a high melting point

A
  • sodium oxide has a giant ionic structure
  • have strong electrostatic forces of attraction between oppositely charged ions
  • requires a lot of energy to break
28
Q

give one limitation to using a dot and cross diagrams

A

doesn’t show the shape/ only two diminsional

29
Q

give one limitation to using a dot and cross diagrams

A

doesn’t show the shape/ only two dimensional

30
Q

define isotope

A

an atom of the same element that has the same number of protons but a different number of neutrons

31
Q

what is the formula to find the relative atomic mass of an element with different isotopes?

A

(mass number x percentage) of isotope 1 +(mass number x percentage) of isotope 2 / 100

32
Q

give the charge of a proton

A

positive charge +1

33
Q

give the charge of a neutron

A

neutral charge 0

34
Q

give the charge of a electron

A

negative charge -1

35
Q

what is the relative mass of a proton?

A

1 m u (atomic mass units)

36
Q

what is the relative mass of a neutron?

A

1 m u (atomic mass units)

37
Q

what is the relative mass of a electron?

A

1/2000 m u (atomic mass units)

38
Q

how are the elements in the parodic table arranged?

A

atomic number / number of protons

39
Q

how are elements with similar properties place in the periodic table?

A

they are placed in groups

40
Q

how did Newlands order his perodic table?

A

by their atomic weight

41
Q

what were the ‘groups’ Newlands ordered his table called?

A

octaves

42
Q

how did Mendeleev order his periodic table?

A

by their atomic weight

43
Q

what are the 2 main differences between Newlands and Mendeleev’s periodic table?

A

1) M predicted elements that hadn’t been discovered yet and left gaps for these undiscovered elements
2) M altered the strict order of atomic weight so their properties could match

44
Q

why are the noble gases unreactive?

A

because they already have full outer shells

45
Q

why was Mendeleev’s table accepted?

A

elements he predicted were discovered and their properties matched his predictions

46
Q

State two key things that Mendeleev did that no one had done before that made his Table work?

A
  • left gaps for elements he believed were yet to be discovered
  • changed from weight order for some elements to put them in groups with elements with similar properties
47
Q

Describe metallic bonding

A

attraction between nucleus of metal atoms in a lattice to the cloud of delocalised outer shell electrons

48
Q

Explain why sodium is soft

A

atoms all the same sizecan slide over each other while maintaining metallic bonding

49
Q

Explain why bromine has a low boiling point

A

weak forces between molecules

50
Q

Sodium reacts with bromine to form sodium bromide. Explain why this reaction takes place in terms of electrons

A

electrons transferred from sodium atoms to bromine atomsin order for all atoms toget stable electron structures of group 0 atoms

51
Q

Explain why sodium bromide has a high melting point

A

strong attraction between positive and negative ions

52
Q

give 2 similarities in physical properties between group 1 metals and transition metals

A

*conduct heat
*conduct electricity
*malleable
*ductile
*shiny when polished

53
Q

give 2 similarities in chemical properties between group 1 metals and transition metals

A

*react with non-metals to form ionic compounds
*form basic oxides

54
Q

give 2 differences in chemical properties between group 1 metals and transition metals

A

*K is (much) more reactive
*Cu forms ions with different charges, K only forms 1+ ions
*Cu forms coloured compounds but K forms white compounds

55
Q

give 2 differneces in physical properties between group 1 metals and transition metals

A

*Cu has (much) higher melting point
*Cu has (much) higher density

56
Q

What method would you use to separate ethanol from a solution of sugar in ethanol

A

distillation

57
Q

What method would you use to separate ethanol from a mixture of water and ethanol (they are miscible liquids)

A

fractional distillation

58
Q

What method would you use to separate water from a mixture of hexane and water (they are immiscible liquids)

A

separating funnel

59
Q

What method would you use to separate iron filings from a mixture of iron filings with water

A

filtration

60
Q

what can we separate?

A

mixtures

61
Q

what does chromatography separate?

A

solid from another soluble solid

62
Q

what does filtration separate?

A

insoluble solids from a solution

63
Q

what does distillation separate?

A

soluble solute from a solution

64
Q

what does evaporations separate?

A

soluble solute from a solution

65
Q

what is the difference between the reason why you sometimes use evaporation to separate and distillation to separate?

A

sometime you need to collect the solvent itself instead of it just evaporating off

66
Q

how is simple distillation different to fractional distillation?

A

SD separates substances with greater difference between boiling points
FD separates substances with boiling points that are closer to each other

67
Q

Lithium, sodium and potassium are all in group 1 of the periodic table. Which of these has the lowest boiling point?

A

The melting points of the group 1 metals decrease as you go down the group.

68
Q
A

GCSE Chemistry (6 decks)

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