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Chemistry > Atomic Structure And The Periodic Table > Flashcards

Atomic Structure And The Periodic Table Flashcards

1
Q

What is chromatography?

A

Chromatography is the separation of soluble substances

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2
Q

How does it work? - CHROMATOGRAPHY

A

Your soluble mixtures will be on paper at a level line. The paper is lowered into a solvent, and some dyes spreads up the paper, at different rates.

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3
Q

Why do the mixtures move? - CHROMATOGRAPHY

A

The different parts of mixtures are attracted to either the paper or the solvent, meaning the mixture separates

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4
Q

How many spots do pure/impure substances make? - CHROMATOGRAPHY

A

A pure substance creates 1 spot

An impure substance creates more than 1 spot

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5
Q

What were John Dalton’s ideas about atoms? - S+B

A

That they were tiny, indivisible spheres

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6
Q

Who discovered the electron and what model did this create? - S+B

A

JJ Thomson, who created the plum pudding model

1909

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7
Q

What experiment did Ernest Rutherford create and what did he find? - S+B

A

He fired positive alpha particles at gold foil. Most went straight through but some were deflected. This led him to suggest the nuclear model

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8
Q

What is the nuclear model? - S+B

A

An atom, with its mass concentrated at the positively charged nucleus

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9
Q

Who discovered the electron? - S+B

A

JJ Thompson

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10
Q

Who discovered neutrons? - S+B

A

James Chadwick - 1932

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11
Q

What is the atomic number? S+B

A

The number of protons in an element

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12
Q

What is the mass number of an element? - S+B

A

The mass number is the number of protons + neutrons in an element

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13
Q

What is an isotope? - S+B

A

An atom with the same number of protons but a different number of neutrons

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14
Q

What is the symbol for relative atomic mass? - PT

A

Ar

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15
Q

What problems did John Newlands’ periodic table have? - PT

A

He didn’t order elements in terms of atomic weight, put multiple elements in the same place, changed positions of elements.

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16
Q

What was good about Mendeleev’s table? - PT

A

It had spaces left for predicted new elements, decided where elements where misplaced, had elements with similar properties in groups.

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17
Q

Name 4 properties of metals - S+B

A

Good electric conductors, high melting points, very dense, strong, shiny, ductile

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18
Q

Name 4 properties of non metals - S+B

A

Low melting point, low density, weak, not ductile, not malleable, poor conductor of electricity

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19
Q

What is Group 0 of the periodic table? + name to properties - PT

A

The noble gases

Single atoms, very low boiling points, VERY UNREACTIVE

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20
Q

What is group 1 of the PT? + name 2 properties - PT

A

Alkaline metals
Fairly low melting points
Low densities
Soft (can be cut by a knife)

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21
Q

What happens when Lithium reacts with water? - Reactions

A

Fizzes slowly

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22
Q

What happens when potassium reacts with water? - Reactions

A

Burns violently with a lilac flame, often explodes

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23
Q

What do halogens exist as? - S+B

A

Molecules (diatomic)

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24
Q

What happens to the melting and boiling points of group 7 element as you go down the group? - S+B

A

It’s boiling point and melting point increase.

Larger molecules, mean stronger intermolecular forces, requiring more energy to break

25
Q

What can more reactive halogens do to less reactive halogens in a solution? - S+B

A

More reactive halogens can replace less reactive halogens

26
Q

Does halogen reactivity increase up or down the group? - PT

A

Up

27
Q

Name 4 properties of transition metals - S+B

A

Can conduct electricity when solid and liquid, shiny when first cut, high densities, high melting points, strong, hard

28
Q

What can transition metals do in terms of ions? - S+B

A

They can form ions with different charges

29
Q

What is the symbol for relative molecular mass?

A

Mr

30
Q

What did John Newlands (1864) discover?

A

Law of octaves-

Arranged elements by atomic weight and found the elements eight apart had similar properties

31
Q

What was the flaw with Newlands theories?

A

Didn’t consider some elements may be undiscovered and so some elements were grouped with elements of different properties.

32
Q

What did Mendeleev do?

A

Realised that an elements mass was related to its physical and chemical properties. Arranged the elements vertically into groups of similar properties.
He left spaces where undiscovered elements would be

33
Q

Which elements did Mendeleev switch around and why?

A

Iodine and tellurium.
With Mendeleev’s theory, iodine should have been before tellurium but to match up iodine’s properties with chlorine and bromine, he switched them round.

34
Q

What did Henry Moseley (1913) do?

A

Suggested that periodic table should be organised by atomic number not atomic weight (this supported Mendeleev’s decision to put iodine after tellurium)

35
Q

Where in an atom are protons found?

A

Found in the nucleus

36
Q

Where in an atom are neutrons found?

A

In the nucleus

37
Q

Where in an atom are electrons found?

A

On the outside of the atom in electron “shells”

38
Q

What is atomic mass?

A

Number of protons + number of neutrons

39
Q

What is the atomic number?

A

The number of protons (-same as the number of electrons)

40
Q

What does the word element refer to?

A

A substance made up of only one type of atom

41
Q

What does the word compound refer to?

A

A substance made of more than one type of atom- chemically joined

42
Q

When an atom becomes an ion, what happens?

A

It becomes charged by losing/gaining electron(s)

43
Q

What charge would an ion be if it lost electron(s)

A

Positive

44
Q

What charge would an ion be if it gained electron(s)

A

Negative

45
Q

What is the word ending for a negative ion?

A

-ide

46
Q

What type of atoms does ionic bonding occur between?

A

Metal + non-metal

47
Q

What does ionic bonding involve?

A

Electrons are TRANSFERRED (moved) between atoms to form charged ions.

48
Q

What type of structure is formed through ionic bonding and why?

A

(Giant) lattice. Oppositely charged ions that are formed attract each other (ELECTROSTATIC attraction).

49
Q

Name four properties of ionic bonding

A
  • High MPt/ BPt
  • dissolve in water
  • conduct electricity when molten/ dissolved
  • very strong
50
Q

What type of atoms does covalent bonding occur between?

A

non-metals

51
Q

What does covalent bonding involve?

A

Electrons are shared

52
Q

Describe simple covalent molecules?

A
  • the MOLECULES have strong covalent bonds within them

- however, there are weak INTERMOLECULAR forces between molecules (low MPt/ BPt and gas at room temperature)

53
Q

Give an example of giant covalent substances

A

Graphite, diamond, silicon dioxide

54
Q

What type of atoms does metallic bonding occur between?

A

One or more metal atoms

55
Q

What does metallic bonding have that other types of bonding do not?

A

Delocalised electrons

56
Q

What do delocalised electrons do?

A

They hold together positive metal ions, carry charge and carry heat.

57
Q

Name properties of metallic bonding

A

Thermal conductor, electrical conductor, high MPt/ BPt

58
Q

What is an alloy?

A

A mixture of two or more elements where one is metal.

59
Q

Which properties can change when alloys are formed?

A
  • MPt and BPt
  • hardness
  • likelihood to rust

Chemistry (11 decks)

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