Periodic Table Flashcards

1
Q

John Newlands

A

Arranged elements by increasing atomic weight

Noticed every eighth element had similar properties and coincided with the triads- law of Octaves

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1
Q

Dimitri Mendeleev

A

Refined Newlands ideas by using all known data for each element and arranging them into groups and periods

Periodic table established when a new element matched his prediction and filled a gap

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2
Q

Johann Döbereiner

A

Arranged elements in a pattern
Linked properties and found some made triads and that atomic weight of triad’s second element was average of the other two

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3
Q

Covalent bonding

A

Non metals combine by sharing electrons

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4
Q

What properties have covalent bonds

A

Low melting points, weak bonds and weak intermolecular forces
Do not conduct electricity

SHARED ELECTRONS

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5
Q

What kind of metals are in group one

Why do they have similar properties

A

Alkali metals

They all have one electron in outer shell

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6
Q

Why are alkali metals stored under oil

A

They react with air and vigorously with water

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7
Q

What colour does a lithium compound give when burned

A

Red

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8
Q

What colour does a sodium compound give when burned

A

Yellow

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9
Q

What colour does a potassium compound give when burned

A

Lilac

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10
Q

What is produced when alkali metals react with water

A

A hydrogen and a hydroxide

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11
Q

In group one are the metals more or less reactive the further down they are

A

More reactive

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12
Q

In group one what happens to boiling and melting points of the alkali metals, the further down they are

A

They both decrease

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13
Q

Why are the elements in group one more reactive the further down in the periodic table they are

A

Elements further down have outer shells further away from the nucleus making it easier for an atom to lose an electron from its shell

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14
Q

Is oxidation loss or gain of electrons

A

Loss

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15
Q

Is reduction loss or gain of electrons

A

Gain

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16
Q

What are non-metals in group 7 known as

How many electrons in outer shell

A

Halogens

Seven electrons in outer shell

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17
Q

Name first four halogens

A

Flourine
Chlorine
Bromine
Iodine

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18
Q

What are the states of flourine, cholrine, bromine and iodine at room temeprature

A

Flourine is a gas
Chlorine is green gas
Bromine is an orange liquid
Iodine is a grey solid

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19
Q

What are flourine, cholrine, bromine and iodine used for

A

Fluorine used in toothpaste
Chlorine sterilises water and makes pesticides and plastics
Iodine sterilises wounds

20
Q

What do halogens react with to make metal halides

A

Halogens react with alkali metals to form metal halides

21
Q

As we go down group 7 are the elements more or less reactive

A

Less reactive

Flourine is most reactive

22
Q

In a water solution of its metal halide, what will a halogen displace

A

A halogen displaces a less reactive halogen, solution forms

Eg. If chlorine is passed through aqueous potassium bromine solution
Bromine is formed due to displacement

23
Q

In group seven what happens to boiling points, melting points and density of the alkali metals, the further down they are

A

They increase

24
Why is flourine the most reactive of the halogens
It is easiest for it to gain the extra electron as the outer shell is closer to the influence of the nucleus
25
What metals are included in transition metals They have typical qualities
``` Iron Copper Platinum Mercury Chromium Zinc ```
26
Compounds of transition metals are often coloured What colour are copper compounds
Blue
27
Compounds of transition metals are often coloured What colour are iron(II) compounds
Grey/green
28
Compounds of transition metals are often coloured What colour are iron (III) compounds
Orange-brown
29
Transition metals and their compounds can be used as catalysts in chemical reactions What are two examples of this
Iron is used in haber process | Nickel is used in manufacture of margarine
30
Thermal decomposition
Substance is broken down into simpler substances by heating
31
When transition metals are heated under thermal decomposition what occurs
Colour change | Decompose to form a metal oxide and carbon dioxide
32
When does limewater turn milky
When carbon dioxide us present
33
What is the reaction between transition metal ions and sodium hydroxide solution called
A precipitation reaction
34
In thermal decomposition of transition metal carbonates, | What are the products of copper carbonate (II)
Copper carbonate(II) = Copper(II) oxide + carbon dioxide
35
In thermal decomposition of transition metal carbonates, | What are the products of iron carbonate (II)
Iron carbonate(II) = Iron(II) oxide + carbon dioxide
36
What can metal compounds in solution form when sodium hudroxide solution is added to them
Precipitates (insoluble solids)
37
Iron is a transition metal what are it's uses
Iron is used to make steel it is very strong Steel used for cars
38
Copper is a transition metal what are it's uses
Copper is a good conductor Used for electrical wiring Used to make brass
39
Give properties of metals
Lustrous eg. For jewellery Hard with high density eg. For drill bits High tensile strength to bear loads High melting and boiling points Good conductors of heat and electricity eg. saucepans and wiring
40
How are metal atoms held together and how are they arranged As metal atoms pack together, what structure do they build
Metal atoms held together by metallic bond Packed closely in regular arrangement As metal atoms pack together they build a structure of crystals
41
Why do metals have high melting and boiling points
Metal held together by strong electrostatic attraction between metal ions and delocalised electrons Lots of energy needed to overcome the strong metallic bonds
42
Why do metal atoms form a metallic bonds when they are packed together
Atoms packed so close the outer electron shells overlap and form metallic bonds The overlap allows electron to be free (delocalised)
43
How can the structure of metallic bonds be described
Closely packed metal ions in a sea of delocalised electrons
44
In metal atoms, how are metals able to conduct electricity
The free movement of delocalised electrons allows metal to conduct electricity Atoms close together and electrons can move from atom to atom
45
At low temperatures some metals can become superconductors Describe a superconductor
A superconductor has very little or no resistance to the flow of electricity
46
Superconductors have low resistance, when is this useful
When you require: A powerful electromagnet eg. Inside medical scanners Very fast electronic circuits eg. Supercomputer Power transmission that does not lose energy
47
Why are superconductors expensive to use
They operate at about -200'c which is costly and impractical We are trying to find one that will work at room temperature