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GCSE chemistry > Topic 1- Atomic structure & the periodic table > Flashcards

Topic 1- Atomic structure & the periodic table Flashcards

1
Q

What is an atom?

A

The smallest part of an element that can exist.

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2
Q

What is an element?

A

An element is a substanve of only one type of atom.

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3
Q

What is a compound?

A

Two or more elements chemically combined in fixed proportions.

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4
Q

Do compounds have the same properties as their constituent elements?

A

No, they have different properties.

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5
Q

What is a mixture?

A

A mixture consists of two or more elements or compounds not chemically combined together.

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6
Q

Does a mixture have the same chemical properties as it’s constituent materials?

A

Yes, it has the same chemical properties.

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7
Q

What are the 5 methods through which mixtures can be seperated? Do they involve chemical reactions?

A

Filtration, crystallisation, simple distillation, fractional distillation and chromatography. They DO NOT involve CHEMICAL REACTIONS!

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8
Q

Describe the plum pudding model.

A

The atom is a ball of positive charge with negative electrons embedded in it.

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9
Q

Describe the Bohr/ Nuclear model. How did it come about?

A

ALPHA PARTICLE EXPERIMENT CONCLUSIONS:
* The mass of the atom was concentrated at the nucleus.
* The nucleus was positively charged.

THE NUCLEAR MODEL:
* Electrons orbit the nucleus at specific distances. The nuclear model came about throough the alpha particle scattering experiment.

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10
Q

What did James Chadwick do?

A

He provided evidence for the existence of neutrons in the nucleus.

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11
Q

State the relative masses and relative charges of the proton, nuetron and electron.

A

RELATIVE MASSES:
* Proton- 1
* Neutron- 1
* Electron- Very small

RELATIVE CHARGES:
* Proton- +1
* Neutron- 0
* Electron- -1

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12
Q

What is the radius of an atom?

A

0.1 nm

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13
Q

What is the radius of the nucleus?

A

1 x 10^-14 of that of an atom.

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14
Q

What do atoms of the same element have nn common?

A

The same number of protons in the nucleus.

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15
Q

What is an isotope?

A
  • Isotopes are atoms of the same element that have a different number of neutrons
  • Isotopes of he same element have the same elctronic structure, so have the same chemical properties.
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16
Q

What are ions?

A

Ions are charged particles. They are formed when an atoms loses/gains electrons.

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17
Q

What are the properties of metals?

A
  • High boiling point
  • Conduct heat & electricity
  • Shiny
  • Malleable
  • High density
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18
Q

What are the properties of non-metals?

A
  • Low boiling/ melting pint
  • Do not conduct heat/ electricity (except graphite)
  • Dull
  • Brittle, not malleable
  • Low density
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19
Q

What is formed when a metal reacts with a non–metal?

A

An ionic compound.

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20
Q

What is formed when a non–metal reacts with a non-metal?

A

A molecular compoound containing covanlently bonded atoms.

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21
Q
A
22
Q

What is a solute?

A

A substance that is dissolved in a solvent.

23
Q

What is a solution?

A

A solute dissolved in a solvent.

24
Q

What is miscible/immiscible?

A

Miscible- Substances that mix together
Immiscible- Substances that do noot mix together

25
Q

What does soluble mean?

A

A substance that can be dissolved ina solvent.

26
Q

What are the collumns of periodic table called?

A

Groups

27
Q

What are the rows of the periodic table called?

A

Periods

28
Q

Are elements in the same group similar?

A
  • They may have similar chemical properties
  • As they have the same amount of outer shell elctrons
29
Q

What do elements in the same period have in common?

A
  • The same number of energy levels.
  • The same number of shells
30
Q

What were elements arranged in order of before the discovery of protons, neutrons & electrons?

A

In order of atomic weight.

31
Q

Why were some elements placed in inappropriate groups?

A

If strict order of atomic weight was followed.

32
Q

What did knowledge of isotopes make it possible to explain?

A

Why order based on atomic weight was not always correct.

33
Q

What did Mendeleev do?

A
  • Leaving gaps for undiscovered elements.
  • He changed the order of some elements based on atomic weight
34
Q

What are a majority of elements?

A

Metals

35
Q

What are elements in group 1 known as?

A

The alkali metals.

36
Q

Sttate the characteristics of alkali metals.

A
  • All have 1 electron in outer shell
  • All have low density
  • All are stored under oil (to prevent reacction with water/oxygen)
  • All are soft
37
Q

How do group 1 elemnts react with non-metals?

A
  • They form ionic compunds
  • Which are soluble white solids
  • Which form colourless solutions

ALL GROUP 1 ELEMENTS REACT IN THIS WAY BECAUSE THEY ALL HAVE 1 ELECTRON IN THEIR OUTER SHELL!

38
Q

How do group 1 elements react with water?

A

They form hydroxides which dissolves to form alkaline solutions.
* They fizz
* They float
* They move around on surface of water
* They melt
* Potassium only: lilac flame

39
Q

How do group 1 elemnts react with oxygen?

A
  • Lithium: Burns with a strong red flame, produces a white solid
  • Sodium: strong orange flame, white solid
  • Potassium: Lilac flame
40
Q

How do group 1 elements react with chlorine?

A

Lithium: White powder produced
Sodium: Burns with a bright yellow flame, clouds of whte powder
Potassium: Same as sodium but more vigorous

41
Q

How does reactivity change moving down group 1? Why?

A

REACTIVITY INCREASES ⬆
* The atoms get larger
* The distance between the nucleus & outer shell electron increases
* The attraction from the nucleus decreases
* So electrons are more easily lost

42
Q

State the characteristics of group 7.

A
  • 7 electrons in outer shell
  • Coloured vapours
  • Diatomic moleules
  • Form ionic salts with metals
  • Form molecular compounds with non-metals
43
Q

State group 7 elements and their states of matter.

A
  • Fluorine (F2)- pale yellow gas 🟡
  • Chlorine (Cl2)- pale green gas 🟢
  • Bromine (Br2)- dark brown liquid 🟤
  • Iodine (I2)- grey solid 🩶
44
Q

What changes occur moving down group 7?

A
  • Higher relative molecular mass
  • Higher m.p and b.p
  • Reactivity decreases- cannot gain an elcetron as easily
45
Q

A more reactive halogen displaces a less reactive halogen from an aqeous solution of it’s salt. Show this.

A

Cl₂ + 2 NaBr → Br₂ + 2 NaCl
* In this reaction, an orange colour of Br₂ would appear

46
Q

Why does a more reactive halogen displace a less reactive halogen from an aqeuos solution of it’s salt?

A
  • Reactivity decreases going down the group
  • The atoms get larger
  • Less attraction between nucleus and outer shell electron
  • The outer shell electron is more easily lost
47
Q

Compare group 1 metals & transition metals.

A

SIMILARITIES:
* Both conduct heat & electricity
* Both are shiny when polished
* Both form ionic compounds with nn-metals

DIFFERENCES:
* Transition metals have higher densities & higher melting points than group 1 metals
* They are less reactive than group 1 metals
* They are harder than group 1 metals

48
Q

Common characteristics of transition metals:

A
  • **Have ions **with different charges
  • Form coloured compounds
  • Are useful as catalysts
49
Q

What is a catalyst?

A
  • A chemical substance that increases the rate of chemical reaction
  • It is not used up over the course of the reaction
50
Q

State the colours of flames observed when lithium, sodium and potassium burn in oxygen.

A
  • Lithium- Crimson
  • Sodium- Yellow-orange
  • Potassium- Lilac
51
Q

Describe the properties of noble gases. Describe the trends going down the group.

A

PROPERTIES:
* Non-metals
* Gases
* Low boiling point
* Unreactive (have a full outer shell)
* Do not easily form molecules (full ouer shell)
* 8 electrons in outer shell

TRENDS GOING DOWN:
* Atoms have a latger relative atomic mass
* So b.p increases

GCSE chemistry (7 decks)

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