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Chemistry > The Periodic Table > Flashcards

The Periodic Table Flashcards

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1
Q

Who was Mendeleev

A

Mendeleev was a Russian scientist. He came up with the idea of organising the elements in a table.

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2
Q

What was special about Mendeleev’s first table of elements

A

Left gaps for undiscovered elements
Arranged elements in groups and periods
Separated metals
Arranged elements in atomic mass.

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3
Q

Why was leaving gaps in Mendeleev’s design so genius?

A

It allowed him to predict the properties of the undiscovered elements accurately.

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4
Q

How is the modern periodic table different to Mendeleev’s original design

A

No gaps
Noble gases
Elements in atomic order
Actinides and lanthanides

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5
Q

Define element

A

A substance which is made up of one type of atom and cannot be broken down into anything simpler by chemical means

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6
Q

What is a period

A

The horizontal rows in the periodic table

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7
Q

What is a group

A

A vertical column in the periodic table

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8
Q

Name properties of metals

A

Good conductors of electricity and heat
High melting and boiling points
All solid at room temperature (except mercury)
Shiny
Malleable
Ductile
Sonorous

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9
Q

Where is the divide between metals and non metals on the periodic table

A

Aluminium steps down to Polonium

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10
Q

Which elements are gases at room temperature

A

Nobel gases
Nitrogen
Oxygen
Fluorine
Chlorine

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11
Q

Which elements are liquids at room temperature

A

Bromine
Mercury

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12
Q

What do elements in each group have in common with each other

A

They all have the same amount of electrons in the outer shell giving them same properties

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13
Q

What elements are in group 1

A

Alkali metals

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14
Q

What trends do elements in group 1 follow down the group

A

Bigger atoms
More dense
Even softer to cut
Lower melting/boiling point
More reactive

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15
Q

Why are the alkali metals more reactive down the group

A

Reactivity increases because of the 1 electron needing to be lost. The further away the outer shell it the easier it is to lose. The easier to lose the more violent reaction.

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16
Q

Which elements are less dense than water

A

First 3 in group 1 (lithium, sodium and potassium)

17
Q

What is the ionic equation for group one metals

A

M—-> M+➕e-

18
Q

What observations are made when lithium is added to water

A

Metal floats, fizzing occurs, heat is released, moves about the surface and disappears with a smoke and crackle/explosion.

19
Q

What observations are made when sodium is added to water

A

Metal floats, fizzing occurs, heat is released, melts into a ball, moves about surface and disappears with a smoke and crackle/explosion

20
Q

What can be observed when potassium is added to water

A

Metal floats, fizzing occurs, heat is released, a lilac flame, moves about the surface and disappears with a smoke crackle/explosion.

21
Q

What are elements in group 2 known as

A

Alkaline Earth metals

22
Q

What are elements in group 7 known as

A

Halogens

23
Q

Why are group 1 metals stored safely in oil

A

To stop oxidisation of elements as they will quickly.

24
Q

Why does the boiling points of the noble gases increase down the group

A

The increased strength of wan der waal forces.

25
Q

What are the element in group 0/8 known as

A

The noble gases

26
Q

What is fluorine’s appearance at room temperature

A

Pale yellow gas

27
Q

What is chlorines appearance at room temperature

A

Pale green gas

28
Q

What is bromines appearance at room temperature

A

Red-brown liquid

29
Q

What is iodines appearance at room temperature

A

Dark grey solid gives off purple vapour

30
Q

What are trends for halogens down the group

A

Bigger atoms
Less soluble
Increasing melting/boiling point

31
Q

What is the test for chlorine

A

Turns damp blue litmus paper / damp universal indicator paper red then bleaches it white.

32
Q

What is the ionic half equation for formation of halogen ions us chlorine as example

A

Cl2 ➕ 2e- —-> 2Cl-

33
Q

How are the transition metals different to those in group 1

A

Higher melting points
Higher density
Less reactive with water
Form ions with different ions (e.g Iron III and iron II)
Form coloured compounds

34
Q

What compounds colour the transition metals

A

Oxide -black
Carbonate -green
Sulfate- blue

35
Q

Recall the observation when solid iodine sublimes

A

I2(solid) —-> I2(gas) purple vapour

Chemistry (10 decks)

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