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Chemistry 9-1 iGCSE Oxford AQA > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

1
Q

What determines the size of an atom?

A

Volume of electron’s orbits

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2
Q

What is radius of an atom?

A

0.1 nano meters

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3
Q

What is the charge of the nucleus and why?

A

Positive charge because protons

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4
Q

What does the nucleus contain?

A

Contains protons and neutrons

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5
Q

Where is almost the whole mass of atom is concentrated?

A

In nucleus

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6
Q

What is no. of protons equal to?

A

no. of electrons

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7
Q

What does the nuclear symbol of atom (i.e. what’s on the periodic table) tell you?

A

Its atomic number and mass number

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8
Q

What a mass number?

A

Total number of protons and neutrons in atom

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9
Q

What’s the atomic number?

A

Number of protons

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10
Q

How do find the no. of neutrons?

A

Mass Number − Atomic Number

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11
Q

What is the name given to substances that only contains atoms with same number of protons?

A

Elements

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12
Q

Define isotopes

A

Different forms of same element, which have same no. of protons, but different no. of neutrons

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13
Q

What is relative atomic mass?

A

Average mass of one atom of an element (including

isotopes)

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14
Q

How are elements laid out in the periodic table?

A

In order of increasing atomic (proton) number

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15
Q

Where are metals & non-metals on the periodic table?

A

Metals are on left and non-metals on right

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16
Q

What does the group number tell you?

A

Number of electrons in outer shell

Exception Group 0 which has Helium (2 electrons)

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17
Q

What do periods show you?

A

New period = another full shell of electrons

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18
Q

What does having one electron on the outer shell do to an atom?

A

Makes them very reactive and gives similar properties

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19
Q

Name 2 properties of Group 1 metals

A

All are soft and have low density

20
Q

As you go down Group 1…. (Name 3 things)

A
  1. Increasing reactivity
  2. Lower melting points
  3. Lower boiling points
    (4. Higher relative atomic mass)
21
Q

Why does reactivity increase as you go down Group 1?

A
  1. Outer shell electron is further away from nucleus, further down the group
  2. ∴ attraction between nucleus and electron decreases
  3. Outer electron is more easily lost
22
Q

What do alkali metals form with non-metals & why?

A

Ionic compounds with charge go +1 - don’t need much energy to remove 1 outer electron to form full outer shell

23
Q

What are ionic compounds formed from alkali metals and non-metals like?

A

Usually white solids that dissolve in water to form colourless solutions

24
Q

Name 3 observations that occur when alkali metals react with water

A
  1. Metal travel quickly along surface of water
  2. Lots of fizzing
  3. Metal gets smaller
  4. Universal indicator turns purple
25
Q

Why does universal indicator turn purple when alkali metals react with water?

A

Salts produced dissolve in water to produce alkaline solutions

26
Q

Name 2 properties of Group 7 elements

A

All Non-Metals with Coloured Vapours

27
Q

What structures do halogen compounds have?

A

Simple molecular (covalent) structures

28
Q

As you go down Group 7, halogens… (name 3 things)

A
  1. Become less reactive
  2. Have higher melting and boiling points
  3. Have higher relative atomic masses
29
Q

Why does the reactivity decrease as you go down Group 7?

A

Harder to gain extra electron = outer shell’s further from nucleus

30
Q

Name 2 properties of Group 0 elements

A

All Inert, Colourless Gases (at room temp)

31
Q

Why are noble gases non-flammable?

A

Bc they’re inert

32
Q

What do noble gases exist as?

A

Exist as monatomic gases (single atoms not bonded to each other)

33
Q

As you go down group 0…

A

Boiling points of noble gases increase

34
Q

Why does the boiling point of noble gases increase as you go down the group (0)?

A

Bc there’s increase in no. of electrons in each atom = greater intermolecular forces between them which need to be overcome

35
Q

Who developed the periodic table?

A

Dmitri Mendeleev

36
Q

What did Dmitri Mendeleev do to the periodic table?

A

Left gaps and predicted new elements

37
Q

What was the order of Mendeleev’s periodic table?

A

Elements mainly in order of atomic mass but switched some to group that had other elements with similar properties

38
Q

What did the gaps in Mendeleev’s periodic table ensure?

A

Elements with similar properties stayed in same groups

39
Q

Why were their gaps in Mendeleev’s periodic table and what did this allow him to do?

A

Gaps indicated existence of undiscovered elements & allow him to predict what properties they may have

40
Q

Where are the transition metals located in the periodic table?

A

In centre of periodic table between group 2 and group 3

41
Q

Name 3 special properties of transition metals

A
  1. Can have more than one ion
  2. Compounds formed are colourful
  3. Make good catalysts
42
Q

Why are compounds formed with transition metals colourful?

A

Transition metal ions = often coloured

43
Q

Give an example of a transition metal used as a catalyst in a named process

A

Iron catalyst used in Haber process

44
Q

Describe how properties of transition metals differ compared to the properties of group 1 metals (name 3 properties)

A
  1. Have higher melting points (expect for mercury) + higher densities
  2. Much less reactive
  3. Are stronger and harder
45
Q

When alkali metals react with water, what do they release?

A

Hydrogen

46
Q

What do alkali metals form and what kind of solutions do they give when dissolved in water?

A

Form hydroxides that dissolve in water to give alkaline solutions

47
Q

Explain why fluorine is the most reactive element in Group 7

A
  • Fewest energy levels in group 7
  • Greatest attraction between nucleus and outer shell
  • ∴ fluorine can gain an electron in its outer shell more easily

Chemistry 9-1 iGCSE Oxford AQA (11 decks)

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