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Chemistry > 2 - Atoms, Elements & Compounds > Flashcards

2 - Atoms, Elements & Compounds Flashcards

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1
Q

Describe the features of Graphite

A

Made from Carbon
- made from layers of carbon atoms
- atoms arranged in hexagons
- strong covalent bonds between carbon atoms
- weak intermolecular forces between layers
- 3 covalent bonds, 1 delocalised electron
- only nonmetal > good conductor of electricity
-layers slide
Uses :
- pencils
- lubricants

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2
Q

Name the types of physical property:
White -
Solid -
801°-
2.17 g/m3 -
1413° -
Soluble in water -
Crystalline -

A
  • Colour
  • state (at room temperature)
  • melting point
  • Density
  • boiling point
  • solubility
  • structure/ appearance
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3
Q

How are electrons distributed in non-water molecules

A

Randomly,
but there is always a place with more electrons than the other, creating + and - charges, and intermolecular forces

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4
Q

What is water’s special property regarding electrons?

A

Electrons NOT evenly distributed
Oxygen attracts more electrons from Hydrogen

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5
Q

Give an example and a non-example of “isotope”

A

H-1, H-2, H-3
__________________________

He is Not isotope of hydrogen

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6
Q

Define Particle

A
  • Building blocks of the universe
  • Portion of matter
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7
Q

Def. nucleus

A

The centre of the atom, composed of protons and neutrons.

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8
Q

Def. electron shell

A

Orbits of electrons circling the nucleus

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9
Q

Def. electron

A

A particle in the atom with a negative charge and relative mass of 0, that orbits the nucleus in electon shells.

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10
Q

Def. proton

A

Positively charged particle in the nucleus of an atom

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11
Q

Def. neutron

A

Neutrally charged particle in the nucleus of an atom

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12
Q

What are the relative charges and masses?
Proton
Electron
Neutron

A

Proton - +1,1
Electron - -1, 0
Neutron - 0,1

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13
Q

Name the first 4 shells and the amount of electrons they contain

A

1st shell - 2
2nd shell - 8
3rd shell - 8
4th shell - 8

Up to atom 20

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14
Q

Give another word for “atomic number”
What is it ?

A

Proton number

(number of protons)
(meaning also electrons)

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15
Q

Give another word for “relative atomic mass”
What is it?

A

Nucleon number

(protons + neutrons)

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16
Q

What is an isotope?

A

Atoms of an element with the same number of protons and electrons,
but a different number of neutrons

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17
Q

What is a covalent bond?

A

An electrostatic attraction between shared electrons and adjacent nuclei

(see paper card for diagram )

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18
Q

What are the characteristics of an ionic compound

A
  • Casually contain a metal + one or two non-metal
  • The solid is an ionic lattice
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19
Q

Give example and non example of molecular substances

A
  • Oxygen O2, Sulfur S2, Hydrogen H2
  • Water H2O, Methane CH4, Carbon dioxide CO2
    ________________________________
    non-examples :
  • ionic compounds like MgO or NaCl
  • Giant covalent structures like diamond
  • metals like sodium or copper
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20
Q

Why is a nitrogen molecule un-reactive?

A

Because it has more bonds, making it more stable
N=_N

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21
Q

Why do molecular solids melt easily?

A

Weak intermolecular forces

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22
Q

Why are most substances made from molecules liquids or gases at room temp.?

A

EMPTY

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23
Q

Why are molecular substances ALWAYS poor conductors of electricity? Except for graphite.

A

EMPTY

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24
Q

What does N2 look like

7
N, 2, 5
14

A

Nitrogen sharing 3 covalent bonds with other Nitrogen

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25
Q

What happens to inter molecular forces as a gas

A

They are still there, but molecules have energy to break free

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26
Q

What is electron configuration of

3
Li+
7

A

2

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27
Q

Define “ionic lattice”

A

A solid formed from cations and anions held together by an ionic bond

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28
Q

Define “ionic bond”

A

Electrostatic attraction between oppositely charged ions

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29
Q

Define Lattice

A

regular arrangement

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30
Q

Al (OH)3 Why brackets?

A

To not confuse between Al + O + 3 x H and Al + O x H x 3

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31
Q

Name the compound NaI

A

Sodium iodide

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32
Q

Name the compound AlPO4

A

Aluminium phosphate

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33
Q

Name Li3N

A

Lithium nitride

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34
Q

What are there
O=O
H-H
N=_N

A

Molecules of :
Oxygen
Hydrogen
Nitrogen

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35
Q

What is electronic configuration? how many protons, neutrons, electrons?
8
O
oxygen
16

A

8,8,8

2.6

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36
Q

11p 2.8,1 18p 2.8.7
10e 17e

What happens?

A

reaction

11p 17p
10e 2.8 — +1 —> 18e 2.8.8

Cation anion
full outer shells!
(to be balanced)

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37
Q

What do you call a positive ion?

A

Cation +

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38
Q

What do you call a negative ion?

A

Anion -

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39
Q

What would a reaction between chlorine and sodium create?

A

NaCl
Sodium Chloride

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40
Q

What a the characteristics of isotopes?

A
  • Atomic number does not change
  • Relative atomic mass can change
  • electron configuration same
  • isotopes have same properties as each other except for mass
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41
Q

What is a polyatomic ion?

A

Ion composed of multiple elements
e.g. SO4, sulphate

42
Q

What is the ratio of cations to anions in NaCl?

A

1:1

43
Q

What is an electronic configuration?

A

A way to represent number of electrons in each shell
e.g. 2,8,3 (Aluminium)

44
Q

What is electron valency?

A

Outer shell

45
Q

What are the patterns in the periodic table?

A

noble gases = full shell
Otherwise, group number = n. of electrons on outer shell
period number = n. of electron shells
Always increasing by 1 proton

46
Q

Name the parts of an atom

A

nucleus, electron, neutron, electron shell, proton

47
Q

12
Mg (78,70%) found in nature
24

12
Mg (10.13%)
25

12
Mg (11.17%)
26

Find Ar

A

(78.7x24) + (10.13x25)
+ (26x11.17)
_____________________________
100 (because per cent)

48
Q

17
Cl How to find Ar?
35.5

25Cl 25Cl

25Cl 27Cl

A

Find mean average

(25)3 + 27
______________ = 35.5
4

49
Q

What is overall charge ?

16p
17e

A

-1

50
Q

How would they react?

    Ca                    F
 2.8.8.2              2.7
A

Ca gives one electron each to 2 F atoms

51
Q

What does Ar stand for?

A

Average relative atomic mass

52
Q

What happens when you try to conduct electricity through a liquid ionic substance

A

The ions transfer electricity by moving towards the electrodes

53
Q

Def. Atom

A

A neutral particle composed of protons, neutrons, and electrons

54
Q

Define ion

A

A particle with a positive or negative charge due to the loss or gain of electrons

55
Q

Define and draw a molecule

A

Two or more atoms joined together by covalent bonds (and it is neutral)

56
Q

easter egg!

A

Coucou! :-)

57
Q

How many covalent bonds does carbon make

A

Alway 4

58
Q

What is simple covalent bonding VS Giant covalent bonding

A
  • set number of atoms bond
  • can have infinite amount of bonds
59
Q

Did you know which atom has an anomaly in non-metal ion names?

A

Carbon
Carbide
Carbonate

60
Q

? +? = 2NaCl

A

2Na + Cl2 = 2NaCl

61
Q

What are the physical properties of ionically bonded substances ?

A
  • high melting point
  • conductive when dissolved/ liquid/ gas
    when ions can move
62
Q

Highlight differences : molecular vs macromolecular

A
  • made of small molecules joined by weak intermolecular forces
  • atoms joined with strong covalent bonds
    _____________________________
    One giant molecule in which ALL atoms are joined together with strong covalent bonds
63
Q

What does immiscible mean?

A

Can’t mix

e.g. oil and water don’t mix

64
Q

What is NH3?

A

Ammonia

65
Q

Def. intermolecular forces

A

Forces (electrostatic attractions) between molecules (weak, easy to break)

66
Q

Def. molecular substances

A

A substance made from molecules that could be a solid, liquid or gas at room temperature

67
Q

What are the general properties of simple covalent molecules?

A

Normally:
- electrical insulator
- low melting point
- gas at room temperature

68
Q

Why is diamond hard ?
Why is graphite soft?
Graphite good conductor of electricity?

A

EMPTY

69
Q

Describe the features of silicon dioxide

A
  • aka: sand, quartz
  • SiO2 simplest ratio of each element (1:2)
  • very high melting point - about 1500°
  • 3D lattice of atoms
  • each silicon makes 4 strong covalent bonds, oxygen makes 2
  • when pure-> transparent
  • uses: glass
70
Q

What are the features of diamond

A
  • Made from carbon atoms
  • each carbon 4 bonds
  • 3D lattice of atoms
  • Transparent
  • extremely hard, almost impossible to scratch
  • melting point 4000°
  • uses : jewellery, drilling (and cutting glass btw)
71
Q

Def. Element

A

Substance made of only one type of atom

72
Q

Def. Compound

A

Substance made of 2 or more elements chemically bonded.
It has a definite composition (you can wite a formula)

73
Q

Def. Mixture

A

Substance made of 2 or more substances physically combined.
It has a variable composition (you cannot write a formula)

74
Q

Def. Solution

A

A mixtrue of one r more dissolved solids (solutes) in to a liquid (solvent)

75
Q

Def. Solvent

A

The larger component of a liquid mixture, a substance that dissolves a solute

76
Q

Def. Solute

A

The smaller component of a lquid mixture, a substance dissolved into into a solvent.

77
Q

Def. Saturated solution

A

A solution containing the maximum concentration of a solute dissolved in a solvent at a specifiesd temperature.

78
Q

Def. Residue

A

The particles left behind in a filter

79
Q

Def. Filtrate

A

The particles that came through a filter

80
Q

Suggest a method to separate mixed salt and pepper

A
  1. Add water to the mixture
  2. Stir and dissolve the salt into a solution (pepper is insoluble)
  3. Pass the mixture through a filter to separate the salt solution from the pepper
  4. Boil the salt solution to get rid of the water
81
Q

What is a solute

A

something dissolved in water

82
Q

What are characteristics of molecular substances

A
  • non-metal atoms that join together with covalent bonds to form molecules
    (share electron —> full outer shells)
  • molecules attracted to each other by weak intermolecular forces
  • Volatile (turn to gases easily)
  • often soluble (in water or other solvent like alcohol)
  • poor conductors of electricity in any form
83
Q

What are the state symbols ?

A

g = gas
l = liquids
s = solids
aq = aqueous : dissolved in H2O

84
Q

Def. Periodic Table

A

An arrangement of elements in periods and groups and in order of increasing proton number/atomic number

85
Q

Describe the change from metallic to non-metallic character across a period

A

Decreases as you move left to right (down a period), while Increases as you go down groups

86
Q

Def. Metal

A

Elements that will form positive ions when they react because they lose electrons.

87
Q

Def. Nonmetal

A

Elements that will form negative ions when they react because they gain electrons.

88
Q

Def. Semimetals/Metalloids

A

Elements that display characteristics of both metals and nonmetals

89
Q

Def. Metallic character

A

Level of reactivity of a metal

90
Q

Def. Nonmetallic character

A

Tendency to accept electrons during chemical reactions

91
Q

Describe the relationship between group number and the charge of the ions formed from elements in that group

A

The group number is equal to the number of electrons in the outer shell, which dictates what kind of ion the atom will form when it reacts. A group 1 ion wil have +1 charge, and a group 2 ion will have a +2 charge, and so on. From group 5 onwards, the charges are -3, -2, and so on.

92
Q

Compare the thermal conductivity of metals and nonmetals

A

Metals are good conductors of heat, while non metals are insulators of heat

93
Q

Compare the electrical conductivity of metals and nonmetals

A

Metals are good conductors of electricity, while non metals are insulators of electricity

94
Q

Compare the malleability and ductility of metals and nonmetals

A

Metals are malleable and ductile while nonmetals are brittle

95
Q

Compare the melting and boiling points of metals and nonmetals

A

Metals have higher melting and boiling points than nonmetals

96
Q

Describe the properties of noble gases

A
  • Unreactive,
  • Monatomic
  • Gas
97
Q

Explain why noble gases are unreactive in the terms of electronic configuration

A

Noble gases have full outer shells so they are stable. This means they do not need to gain or lose lelectons to increase their stability.

So all other atoms react to get noble gas-like, full outer shells

98
Q

What happens in metallic bonding?

A

Each metal electron in the outer shell becomes delocalised form the atom, leaving a cation. The electrons can move freely between different ions, forming a sea of delocalised electrons.

99
Q

Why is there a strong electrostatic attraction in metallic bonds?

A

The negative delocalised electrons are attracted to the positive metal ions.

100
Q

How many electrons are there in a sea of electrons in a metallically bonded substance?

A

A number equal to the amount of positive charges of the cations

So the overall charge its neutral

Chemistry (12 decks)

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