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Chemistry Flashcards

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1
Q

What charge does a neutron have?

A

Neutral

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2
Q

What charge does an electron have?

A

Negative

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3
Q

Electron configuration

A

2,8,8

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4
Q

Atomic mass=

A

protons + neutrons

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5
Q

First 20 elements

A 
Hydrogen
Helium
Lithium
Beryllium
Boron
Carbon
Nitrogen 
Oxygen
Fluorine
Neon
Sodium
Magnesium
Aluminium
Silicon
Phosphorus 
Sulphur
Chlorine
Argon
Potassium
Calcium
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6
Q

Chemical elements for hydrogen

A

H

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7
Q

Chemical element for helium

A

He

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8
Q

Chemical element for lithium

A

Li

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9
Q

Chemical element for beryllium

A

Be

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10
Q

Chemical element for boron

A

B

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11
Q

Chemical element for carbon

A

C

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12
Q

Chemical element for nitrogen

A

N

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13
Q

Chemical element for oxygen

A

O

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14
Q

Chemical element for fluorine

A

F

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15
Q

Chemical element for neon

A

N

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16
Q

Chemical element for sodium

A

Na

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17
Q

Chemical element for magnesium

A

Mg

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18
Q

Chemical element for aluminium

A

Al

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19
Q

Chemical element for silicon

A

Si

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20
Q

Chemical element for phosphorus

A

P

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21
Q

Chemical element for Sulfur

A

S

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22
Q

Chemical element for Chlorine

A

Cl

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23
Q

Chemical element for Argon

A

Ar

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24
Q

Chemical element for potassium

A

K

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25
Q

Chemical element for calcium

A

Ca

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26
Q

What charge does a proton have?

A

Positive

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27
Q

Electric Charge for a nucleus

A

Positive

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28
Q

Electric Charge for an atom

A

Neutral

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29
Q

Formula for Electrons

A

2n squared

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30
Q

Put protons, atoms, electrons and neutrons in order of lightest to heaviest

A

Electrons, Protons, Neutrons, Atoms

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31
Q

How many elements are there?

A

118

32
Q

Ion

A

Is an atom that has gained or lost its valance electrons.

33
Q

When atoms gain an electron what charge do they obtain?

A

Negative Charge

34
Q

What charge do atoms obtain when they loose an electron?

A

Positive

35
Q

What is the name for a positively charged electron?

A

Cation

36
Q

What is the name for a negatively charged atom?

A

Anion

37
Q

What is an isotope?

A

An atom with the same number of protons but differing number of neutrons than per usual this altering the atomic mass.

38
Q

What is another word for electron shells?

A

Energy Levels

39
Q

Element Defintion

A

A substance composed of atoms with the same atomic number. The most pure form of substance.

40
Q

Ground State-Defintion

A

Lowest energy arrangement of an atoms electrons in energy shells.

41
Q

What direction do the groups on the periodic table go?

A

Vertically

42
Q

What direction do the periods on a periodic table go?

A

Horizontal

43
Q

How can it be figured out which group an element is in?

A

The number of electrons in the valance shell

44
Q

How can it be figured out with period the element is in?

A

How many electron shells that the element has.

45
Q

Define covalent bonding.

A

The sharing of electrons between non-metallic elements. They bond with each other to form a new substance and fill each other outer shell so that the shell is satisfied.

46
Q

What two types of elements is covalent bonding between?

A

Non-metallic elements

47
Q

What two types of elements is ionic bonding between?

A

Metal and Non-Metal elements

48
Q

Valance Shell Defintion

A

The last electron shell of an element, this shell will contain the highest energy level.

49
Q

How can electrons jump for shell to shell?

A

If electrons are provided with more energy they move away from the nucleus further out and they jump from inner shells to outer shells.

50
Q

How many valance electrons do the Nobel gases have?

A

None they are satisfied elements.

51
Q

What causes a positively charged atom to be like this?

A

More protons then electrons.

52
Q

What causes a negatively charged atom to be like this?

A

More electrons than protons

53
Q

Which type of elements are most likely to loose electrons?

A

Metallic

54
Q

Which type of elements are most likely to gain electrons?

A

Non-Metallic

55
Q

Explain and Define Ionic Bonding

A

Metallic elements loosing and electron and transferring them to a non-metallic element so that each element has a full set.

56
Q

Which type of element is the most reactive?

A

Metallic

57
Q

Which type of elements does metallic bonding occur between?

A

Metal and Metals

58
Q

Fill in the blanks

Metal atoms ________ electrons to form ________ ions which have more ________ than _______.

A

Loose
Positive
protons
Electrons

59
Q

Fill in the blanks

Non-metal atoms _________ electrons to form __________ ions which have more ________ than protons

A

Gain
Negative
Electrons
Protons

60
Q

Why are metals such good conductors of electricity?

A

They have a weak structure so electrons can be free moving. a the see of free electrons allow metals to carry electrical currents.

61
Q

Whittier are electrons attracted to?

A

As electrons are negatively charged they are attracted to the positive protons, in the nucleus. This keeps the electrons in orbit.

62
Q

Which shell is most attracted to the nucleus?

A

The first one, as its closest which makes it the lowest energy

63
Q

When do electrons have the highest energy?

A

When they are in the outer shell. They have less of an attraction to the nucleus.

64
Q

What is a firework?

A

The explosion energy causes the electrons to jump shells. As they return to the ‘ground state’ energy gets released as light

65
Q

What is a chemical formula?

What does this chemical formula tell you H20?

A

A formula that tells you what elements make up the substance and in what proportions.
In H2O
There are 2 hydrogens bonded to an oxygen.

66
Q

What’s bigger? Protons or Neutrons

A

Neutrons slightly

67
Q

Monatomic

A

Atoms that exist on their own, without bonding with others.

68
Q

What is a lattice and how is it formed?

A

A lattice is formed when electrostatic forces are pulled together to form a strong ionic bond. Each ion is surrounded by an opposite charge that it is being attracted to building up a three dimensional structure known as a lattice.

69
Q

What type of force pull negative and positive ions together?

A

Electrostatic

70
Q

What number group is the Nobel gases and what is so special about them?

A

They are number 18 and then are monatomic atoms, known for their intense stability.

71
Q

Do metal atoms have a strong or weak bond in regards to their electrons?

A

Weak

72
Q

Do non- metal atoms have a strong or weak bond in regards to their electrons?

A

Strong

73
Q

What group would an atom be that had an electron configuration of 2,8,7?

A

7

74
Q

What period would an atom that had an electron configuration of 2,8,18,8,2 be situated in?

A

5

75
Q

Name two forms of carbon that are lattice structures?

A

Diamond and Graphite

76
Q

Explain why Nobel gases tend not to form bonds?

A

Because they are stable and are satisfied as the occupy full outer electron shells.

77
Q

If an atom has an electron configuration of 2,6 (oxygen) how many covalent bonds will it need to be satisfied?

A

2

General science (4 decks)

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