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Edexcel GCSE Chemistry Triple > The Periodic Table > Flashcards

The Periodic Table Flashcards

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1
Q

Who created the periodic table and when? How many elements did they sort ?

A

Dmitri Mendeleev in 1869 sorted 50 elements into what is known as the periodic table today.

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2
Q

How did Mendeleev sort the table?

A

By order of atomic mass while also placing elements with similar chemical properties in columns (groups).

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3
Q

How could he predict future elements?

A

The order meant that many gaps were left which meant that we could predict the properties of undiscovered elements.

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4
Q

Periodic table

A

A table of all known elements

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5
Q

How many elements do we think there are now?

A

100 (still discovering them now)

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6
Q

How do modern periodic tables order their elements?

A

Increasing atomic number

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7
Q

What does a group tell you?

A

Their properties and number of electrons in their outer shell.

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8
Q

What do periods tell you?

A

How many electron shells

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9
Q

Where’s the partition between metals and nonmetals on the periodic table?

A

Boron to astatine staircase

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10
Q

What’s on the left of the staircase?

A

Metals

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11
Q

What’s on the right of the staircase?

A

Nonmetals

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12
Q

Properties of metals

A

Conduct heat and electricity, sonorous, malleable, shiny, ductile

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13
Q

What’s a characteristic of a metal oxide?

A

They are basic, so will neutralise acids

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14
Q

What’s a property of a nonmetal oxide?

A

Acidic and will neutralise bases

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15
Q

What group are alkali metals? How does this affect their characteristics?

A

1, meaning there is only one outer shell electron. This means that they are very reactive as they readily donate their outer electron to maintain a full outer shell.

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16
Q

Alkali metal + water

A

> metal hydroxide + hydrogen

17
Q

What are the properties of alkali metals?

A

They are soft (low density), have a low bp/mp and are dull coloured.

18
Q

What happens as you go down group 1? Why?

A

Alkali metals increase reactivity, density & bp. This is because the bigger the atom is, the further the outer electron is from the nucleus. This means that there’s less force of attraction and so it is easier to remove the outer electron and so is more reactive.

19
Q

Write out the balanced symbol equation for the reaction between potassium and water.

A

2K + 2H2O > 2KOH + H2

20
Q

What type of reaction is the reaction of water and alkali metals?

A

It’s an exothermic reaction and the flame is the hydrogen on fire.

21
Q

Why do the products of alkali metals and water turn out alkaline?

A

Because it produces a metal hydroxide.

22
Q

What group are halogens?

A

7

23
Q

What happens as you go down group 7?

A

They become less reactive, darker, more dense and higher bp/mp

24
Q

Halogen properties

A 
Low BP’s/MP’s
Toxic, bleaching agents
Nonmetals
Disinfectants 
Very reactive
Diatomic
25
Q

What bonding joins group 7 diatomic molecules?

A

Covalent

26
Q

What does chlorine look like? What’s it used for? Where’s it found?

A

It’s a yellow/green gas found in the ocean/ earth’s crust. It’s used as a water purifier.

27
Q

What does bromine look like? What’s it used for? Where’s it found?

A

It’s a brown/orange liquid that gives off orange vapour. It’s found in the ocean/ earth’s crust. It’s used as a disinfectant.

28
Q

What does iodine look like? What’s it used for? Where’s it found?

A

It’s a grey solid giving off purple vapour. Found in oceans/minerals. It’s used to sterilise/ prevent radiation.

29
Q

What’s the chemical test for chlorine?

A

Has sharp, choking smell. Makes damp, blue litmus paper turn red and then bleach white.

30
Q

Metal + halogen

A

> metal halide (salt)

31
Q

Write out the balanced equation of chlorine + sodium

A

2Na + Cl2> 2NaCl

32
Q

Halogen + halide

A

> hydrogen halide

33
Q

Write out the balanced equation of chlorine + hydrogen

A

Cl2 + H2 > 2HCl

34
Q

Why does HCl form an acid when dissolved?

A

Because it disassociates into H+ & Cl- when in water

35
Q

Hydrogen halide + water

A

> acid

36
Q

Metal halide + water

A

> acid

Edexcel GCSE Chemistry Triple (14 decks)

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