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Science Book 1 > Part 1 > Flashcards

Part 1 Flashcards

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1
Q

Maximum number of electrons that can find in the first three energy levels

A

2,8,8

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2
Q

What does the group number tells you about the electron structure

A

Number of electrons in the outermost shell

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3
Q

What does the period number tell you about the electron structure

A

Number of shells

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4
Q

What is an isotope

A

Element with the same number of electrons and protons, but different number of neutrons

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5
Q

Equation for relative atomic mass (Ar)

A

( (% X mass) + (% X mass) ) divided by 100

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6
Q

How can new experimental evidence affect a model

A

Scientific model being changed

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7
Q

Describe John daltons model of the atom

A

Tiny spheres

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8
Q

Describe JJ Thompsons plum pudding model

A

A ball of positive charge white negative electrons embedded

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9
Q

Rutherfords alpha scattering experiment. Describe the conclusion

A

Atom has a dense, positive centre surrounded by empty space

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10
Q

How did Niels Bohr’s contribute to the atomic model

A

Electrons orbit the nucleus

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11
Q

James Chadwick’s contribution to the atomic model

A

Proved neutrons existed

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12
Q

How are elements in periodic table arranged

A

Increasing atomic number

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13
Q

Describe how scientists before ordered it

A

Atomic weights

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14
Q

What did Mendeleev do to contribute to the modern periodic table

A

Left gaps for undiscovered elements and change the order they where put in

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15
Q

Atoms in Pure metals are arranged…

A

In regular rows

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16
Q

Atoms in pure metals are…

A

Same size

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17
Q

Atoms in alloys are…

A

Varying size because more than one type of atom is present

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18
Q

Atoms in alloys are arranged…

A

Irregularly

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19
Q

Atoms that are in regular rows can…

A

More easily slide over each other

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20
Q

What is an alloy

A

Solid mixture containing at least one metal

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21
Q

Halogens all have…

A

Low melting and boiling points

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22
Q

Fluorine is…

A

Pale yellow gas at Room temp

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23
Q

Chlorine is…

A

Green gas at room temp

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24
Q

Bromine is…

A

Brown/orange liquid at room temp

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25
Q

Iodine is…

A

Purple solid at room temp

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26
Q

What is another word for unreactive

A

Inert

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27
Q

What happens when you go down the noble gas group to the boiling point

A

Increases

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28
Q

What’s normally produced by a chemical reaction

A

Gases

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29
Q

How to know if carbon dioxide is present

A

Turns limewater cloudy, when bubbled through

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30
Q

How to know if oxygen is present

A

Causes glowing splint to relight

31
Q

How to know if hydrogen is present

A

A lit splint to burn with a squeaky pop

32
Q

How to know if chlorine is present

A

Bleaches damp litmus paper

33
Q

What is the most stable electronic arrangement for an atom

A

Full outer shell

34
Q

State the definition of an ion

A

A particle with positive or negative charge

35
Q

Define ‘ionic compound’

A

An electronic attraction between two oppositely charged ions

36
Q

Describe an ionic lattice

A

A giant structure formed by all ionic compounds in which there are strong electrostatic forces of attraction in all directions between oppositely charged ions

37
Q

State the definition of polyatomic ion

A

A charged molecule containing more than one atom

38
Q

How many dimensions are giant ionic lattices

A

Three dimensions

39
Q

Arrangement of ions in giant ionic lattices

A

Regular arrangement of atoms ions in lattice

40
Q

What is the force of oppositely charged ions

A

Electrostatic force of attraction

41
Q

How does the strength of the force relate to the physical properties of ionic compounds

A

All ionic lattices have high melting and boiling points

42
Q

Do ionic solids conduct electricity

A

NO

43
Q

Do molten ionic compounds conduct electricity

A

Yes

44
Q

Do dissolved ionic compounds conduct electricity

A

Yes

45
Q

State the definition of a covalent bond

A

A strong bond between two non-metals formed by a shared pair of electrons

46
Q

State the definition of a molecule

A

Two or more atoms bonded together

47
Q

Describe a simple covalent molecule

A

Small covalent molecules have less than 10 atoms

48
Q

State the state of simple covalent molecules at room temperature

A

Gases or liquids

49
Q

Define intermolecular forces

A

The forces between molecules

50
Q

Describe the intermolecular forces between simple covalent molecules

A

Weak

51
Q

State how the strength of intermolecular forces changes fire to the size of the molecule

A

The bigger the size the forces increase

52
Q

Why can’t Simple covalent molecules conduct electricity

A

There are no charged particles

53
Q

How is graphene formed

A

From one single layer of graphite

54
Q

What sort of structure is graphene

A

One atom thick
Very strong covalent bonds
Hexagonal rings of carbon atoms

55
Q

What are fullerenes

A

Covalent molecules of carbon which have hollow arrangements

56
Q

What is Buckminsterfullerene

A

A molecule of 60 carbon atoms forming hollow sphere

57
Q

Define nanometre

A

1 billionth of a metre

58
Q

Define nanotube

A

Very small tubes made from carbon fullerenes

59
Q

What are metallic bonds

A

Bonds between metal atoms

60
Q

What will metal atoms always lose which causes what

A

Electrons, causing them to gain a positive charge.

61
Q

What is a delocalised electron

A

An electron which is displaced from the outer shell

62
Q

In metallic bonding what do the atoms donate, which forms what

A

Their electrons to form a delocalised sea

63
Q

Positive ions are held by what to attract the delocalised electrons

A

Strong electrostatic force

64
Q

Metallic compounds are good conductors of…

A

Heat and electricity

65
Q

Define ion

A

Particle with a positive and negative charge

66
Q

How do atoms become ions

A

By gaining or losing electrons

67
Q

How do metals form ions

A

Lose electrons to from positive ions

68
Q

How do non-metals typically form ions

A

Gain electrons to form negative ions

69
Q

How do atoms become stable

A

Gaining a full outer shell

70
Q

What is the law of conservation of energy

A

Energy can’t be destroyed or created

71
Q

State units of energy

A

Joules (j)

72
Q

State the right stores of energy

A

Chemical, kinetic, gravitational potential, elastic potential, thermal, magnetic, electrostatic, nuclear

73
Q

What are the four ways energy is transferred

A

Electrically, heating, radiation, work done by force

Science Book 1 (1 decks)

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