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Chemistry X > The Periodic Table - Unit 1 Topic 6 > Flashcards

The Periodic Table - Unit 1 Topic 6 Flashcards

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1
Q

Who first created a table of elements?

A

Newlands

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2
Q

How did Newlands organise elements in order?

A

Increasing atomic mass

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3
Q

What was Newlands’ table of elements called?

Why?

A

Newlands’ Octaves

Similarities between each 8th element

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4
Q

How did Mendeleev create his periodic table?

A

Wrote information about each element on a card and arranged them in piles with similar properties.

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5
Q

How did Mendeleev organise his periodic table?

A

Increasing atomic mass

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6
Q

How many elements did Mendeleev have?

A

63 elements

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7
Q

What are the differences between Mendeleev’s table and ours? (nowadays)

A

No gaps

Noble gases

Actinides & lanthanides

Elements in increasing atomic number

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8
Q

How many elements are there now?

A

118 elements

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9
Q

What are the similarities between Medeleev’s table and ours?

A

Separate metals & non-metals

Arranged in groups & periods

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10
Q

How do atoms change across a period?

Why?

A

Decrease in size

Extra positive charge as extra electron is added, shells pulled closer to nucleus with extra attraction.

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11
Q

Metal + water ->

A

Metal hydroxide + hydrogen

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12
Q

Metal + oxygen ->

A

Metal oxide

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13
Q

Metal + acid ->

A

Salt + hydrogen

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14
Q

Metal + halogen ->

A

Metal halide

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15
Q

What group are alkali metals?

Properties of alkali metals (down group)

A

Group 1

Bigger atoms

More reactive

Denser & softer to cut

Lower melting & boiling point

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16
Q

Why are atoms more reactive? (down the group - alkali)

A

Electrons are further away from the nucleus so they can leave more easily & react/bond.

17
Q

Why do atoms become larger? (down group - alkali)

A

More layers

18
Q

What group are alkaline earth metals?

Properties?

A

Group 2

Bigger atoms

More reactive

Denser & softer to cut

Lower melting & boiling point

19
Q

4 things you would observe when potassium reacts with water?

A

Fizzes

Gives off hydrogen

Moves across surface & disappears

Burns with lilac flame

20
Q

3 things you would observe when sodium reacts with water?

A

Melts into ball & disappears

Gives off hydrogen

Floats on surface

21
Q

Why do atoms have similar properties?

A

Their atoms have the same amount of electrons in the outer shells.

22
Q

Formula for half equations?

A

Metal -> metal + electron

Non-metal + electron -> Non-metal ion

23
Q

Where are the transition metals?

A

In the middle

24
Q

What group are the halogens?

Properties? (up group)

A

Group 7

Smaller atoms

More reactive

More soluble

More reactive

Lower melting & boiling point

25
Q

What group are the noble gases?

Properties?

A

Group 8/0

Unreactive & stable

Denser as you go down

26
Q

Colours:

Fluorine

Chlorine

Bromine

Iodine

A

Colourless (gas)

Pale green (gas)

Red/Brown (liquid)
Purple (solid)

27
Q

Properties of chlorine

A

Slightly soluble in water

Toxic

Denser than air

Bleaches damp litmus paper

28
Q

Source of chlorine?

Uses of chlorine?

A

Electrolysis of Sodium Chloride (Brine)

Water sterilisation

Bleach

Manufacture of PVC

29
Q

What is a displacement reaction?

A

More reactive halogen displaces less reactive halogen from its salt.

30
Q

Properties of metals?

A

Shiny

Malleable

Conducts heat

Conducts electricity

31
Q

What transition metals are used in catalytic converters?

A

Palladium

Rhodium

32
Q

Bromine water + Potassium iodide colour change?

A

To orange/brown

33
Q

What 2 elements are liquid?

A

Bromine

Mercury

34
Q

What elements are gases?

(group & other)

A

Noble gases

Fluorine, & chlorine

Oxygen

Nitrogen

Hydrogen

Chemistry X (28 decks)

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