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Poppy > The Periodic Table > Flashcards

The Periodic Table Flashcards

1
Q

How did scientist try to classify elements in the 19th century?

A

Based on properties and atomic weights

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2
Q

What did new land propose in 1863?

A

His law of octaves; similar properties are repeated every eighth element, he put the elements know at the time into 7 groups based on atomic weight.

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3
Q

Why were new lands ideas not accepted

A

After calcium the properties did not match very well within the groups

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4
Q

Why was mendeleevs table better than newlands

A

The elements fitted better in the groups as he left gaps for undiscovered elements

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5
Q

Why did scientists readily accept mendeleevs ideas?

A

He predicted the properties of missing elements and these were confirmed when the elements were discovered

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6
Q

What did scientist know and not know in the 19th century?

A

They had discovered many elements but did not know about the structure of the atom

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7
Q

When did scientists find out about protons and electrons?

A

The start of the 20th century

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8
Q

Why do elements in the same group have similar chemical properties?

A

They have the same number of electrons in their highest energy level

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9
Q

How are the elements arranged now?

A

In order of increasing atomic number and are arranged in vertical groups

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10
Q

Within a group what does the reactivity depend on?

A

The total number of electrons

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11
Q

Going down the group, there are ……… Energy levels occupied and so the atoms get …….

A

More

Larger

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12
Q

As the atoms get larger what happens to the attraction between the nucleus and the electrons in the highest occupied energy level?

A

The electrons in the highest occupied energy level are less strongly attracted to the nucleus

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13
Q

What is the trend in reactivity of metals?

A

The reactivity of metals increases going down the group

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14
Q

How do metals react

A

By losing electrons

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15
Q

Why do metals get more reactive going down the group

A

To react, metals lose electrons. As the atoms get larger there are more occupied energy levels and the electrons in the highest occupied level are less strongly attracted by the nucleus and so are lost more easily

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16
Q

How do non metals react

A

Gaining electrons

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17
Q

What is the trend in reactivity of non metals

A

The reactivity decreases down the group

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18
Q

Why does the reactivity of non-metals decrease going down the group

A

As you go down the group, the number of occupied energy levels (filled shells) increases. The higher the energy level of the outer electrons, the greater the distance from the nucleus, and the less easily electrons are gained. This is why elements in Group 7 become less reactive as you go down the group

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19
Q

What are group 1 elements called

A

Alkali metals

20
Q

What do the alkali metals react readily with

A

Air and water

21
Q

What are the boiling points & melting points of alkali metals like

A

They are soft solids at room temperature with low melting and boiling points that decrease down the group

22
Q

What are the densities of alkali metals like

A

Low

23
Q

What do alkali metals produce when reacting with water

A

Hydrogen and metal hydroxides

24
Q

What do alkali metals react with to form colourless salts

A

The halogens

25
Q

What do alkali metals dissolve in water to form

A

Solutions that are colourless

26
Q

Why does reactivity increase going down the group of the alkali metals

A

Because the outer electron is less strongly attracted to the nucleus as the number of occupied energy levels increases and the atoms get larger

27
Q

Why is think less reactive than sodium

A

Lithium atoms are smaller than sodium, they have fewer occupied energy levels. Their outer electron is more strongly attracted by the nucleus and so is less easily lost when they react

28
Q

What are the boiling and melting points of transition metals like compared to alkali metals

A

Except for Mercury they have higher mp and bps

29
Q

What 3 properties do transition metals have

A

Malleable
Ductile
Good conductors of heat and electricity

30
Q

What are metal reactions like

A

Slow, not at all or with air or water at normal temperatures

31
Q

How are metals often used

A

Most are strong and dense and are useful as building materials, often as alloys

32
Q

What are the charges of the transition metals

A

Positive ions with various charges

33
Q

What do metal compounds look like

A

Brightly coloured

34
Q

What else are transition metals and their compounds used for in chemical reactions

A

Catalyst

35
Q

Why do halogens have low bps and MPs

A

They have small molecules

36
Q

How do the bps and MPs change in the group

A

They have low bps and mps which increase going down the group

37
Q

What colour is fluorine what state

A

Pale yellow gas

38
Q

What colour is chlorine what state

A

Green gas

39
Q

What colour is bromine and what state

A

Red-brown liquid

40
Q

What state and colour is iodine

A

Grey solid which easily baptised to a violet gas

41
Q

What is formed when halogens ironically bond

A

They form halide ions with a - charge

42
Q

What is formed when halogens covalently bond

A

Molecules are formed

43
Q

What is the reactivity trend in the halogen group

A

Reactivity decreases going down the group

44
Q

A …… Reactive halogen is able to …….. A ………. Reactive halogen from an …….. Solution of a halide compound

A

More
Displace
Less
Aqueous

45
Q

Why does the reactivity decrease going down group 7

A

The attraction of the outer electrons to the nucleus decelerates as the number of occupied energy levels increases

Poppy (12 decks)

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