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Year 10 Chemistry > Unit 2 Chemistry > Flashcards

Unit 2 Chemistry Flashcards

1
Q

What are the columns on the periodic table called?

A

Groups

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2
Q

What are the rows on the periodic table called?

A

Periods

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3
Q

What does the group number an atom is in indicate?

A

It indicates the number of electrons on the atoms outer shell (number of valence electrons)

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4
Q

What does the period number an atom is in indicate?

A

It indicates the number of electron shells an atom has

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5
Q

Will elements in the same group be similar or different chemically?

A

Elements in the same group will have similar chemcial properties due to them having the same number of electrons in its outer shell

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6
Q

How are elements arranged in the periodic table in order of atomic number?

A

They are arranged in increasing order of atomic number (left to right) and this arrangement places elements with similar properties in the same groups

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7
Q

Name all the 7 diatomic molecules

A

1) Hydrogen
2) Nitrogen
3) Oxygen
4) Flourine
5) Chlorine
6) Bromine
7) Iodine

Note:
- Basically ALL of group 7 except for astatine
- Also includes: Hydrgoen, Nitrogen, Oxygen that you need to memorise

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8
Q

What does the oxide of an element mean?

A

The compounds formed when the element reacts with oxygen

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9
Q

What type of oxides do metals form?

A

Metals form basic oxides when reacting with oxygen

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10
Q

What do basic oxides form when they react with acid?

A

Salt and water

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11
Q

What type of oxides do non-metals form?

A

Non-metals form acidic oxides

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12
Q

What do acididc oxides form when they react with bases?

A

Salt and water

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13
Q

What does inert mean?

A

It is when a substance is chemically unreactive

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14
Q

What are electrostatic forces of attraction?

A

The strong forces of attraction between OPPOSITELY charged ions

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15
Q

What does malleability mean?

A

It is the ability of metals to be deformed or moulded into various shapes without breaking, due to movement of atoms in the lattice

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16
Q

What does ductillity mean?

A

Ability of metals to be drawn into wires

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17
Q

Name 3 properties of metals

A
  • Good conductors of electricity
  • High melting and boiling points
  • Malleable
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18
Q

Name 3 properties of non-metals

A
  • Poor conductors of electricity
  • Low melting and boiling points
  • Brittle (break and shatter easily)
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19
Q

What TYEPE of elements are involved in a metallic bond?

A

Metals ONLY

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20
Q

What is a metallic compound?

A

The chemical compound (entire structure) consisting of cations which are bonded to the delocalised electrons throughout the structure by metallic bonding

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21
Q

What is a metallic bond?

A

They are the bonds present in metals formed by the electrostatic forces of attraction between positive metal ions (cations) and delocalised electrons

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22
Q

What are delocalised electrons?

A

Electrons from the outershell of metal atoms that are free to move within the metallic strucutre

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23
Q

How do delocalised electrons in a metallic compound help the metal? (name 2 ways)

A
  • They create the strong forces of attraction that hold the metal together as the elctrons are free to move
  • They also allow for great electric conductivity as they can carry a charge through the structure using delocalised electrons
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24
Q

What happens to the valence electrons of the metals atom in a metallic structure?

A

Atoms lose their valence electrons, which form cations and the lost electrons become delocalised and are free to move throughout the structure

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25
Q

What is the definiiton of an alloy?

A

A mixture of 2 or more metals, or a metal and non-metal combined

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26
Q

What are 2 uses of alloys?

A
  • To enhance the durability of material
  • To increase the strength of material
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27
Q

Why can metallic compounds conduct electricity so well?

A

Because metallic compounds consist of moving electrons (delocalised electons) which can carry a charge therefore allowing electric conductivity

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28
Q

Why do metallic compounds have high melting and boiling points?

A

This is because metallic compounds have strong electrostatic forces of attraction holding the cation with delocalised electrons, this means that it will require more energy to overcome these forces of attraction and break them

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29
Q

What TYPE of elements are invloved in an ionic bond?

A

Metals + Non-metals

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30
Q

What is an ion?

A

An atom or molecule with an electric charge due to the loss or gain of electrons

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31
Q

What is a cation?

A

Positively charged ions formed when an atom loses electron(s)

32
Q

What is an anion?

A

Negatively charged ions formed when an atom gains electron(s)

33
Q

What is an ionic compound?

A

The chemical compound consisting of oppositely charged ions (positive cations and negative anions) that are held together by strong electrostatic forces of attraction

Note: The cations and anions are not specifically bonded to eachother as pairs (they can bond with any other cation and anion)

34
Q

What is an ionic bond?

A

It is the electrostatic force of attraction between oppositely charged ions formed when a metal loses electron(s) to become a positively charged cation and a non-metal gains electron(s) to become a negatively charged anion

35
Q

Can ionic compounds conduct electricity in solid form?

A

No, they cant

36
Q

Why cant ionic compounds conduct electricity in solid form?

A

They cannot conduct electricity in solid form because the ions only vibrate so they cannot carry an electrical charge

37
Q

Why can ionic compounds conduct electricity in liquid form (when melted)

A

Because the ions can move in liquid form (the bonds are broken) meaning the ions can now carry a charge

38
Q

Why do ionic compounds have high melting and boiling points?

A

This is because ionic compounds have strong electrostatic forces of attraction holding the oppositely charged ions (cation and anion), this means that it will require more energy to overcome these forces of attraction and break them

39
Q

What TYPE of elements are involved in a simple covalent bond?

A

Non-metals ONLY

40
Q

What are intermolecular forces?

A

The weak forces of attraction between MOLECULES in a simple covalent compound

41
Q

What are some other names of simple covalent structures?

A

Simple molecules or simple molecular structures (they are the same EXACT thing as simple covalent structures)

42
Q

What is a covalent bond?

A

A strong bond formed when 2 atoms share one or more pairs of electrons to achieve a full outershell

43
Q

How are covalent bonds formed?

A

They are formed when 2 non-metals share and pair their valence electrons between the 2 atoms

44
Q

What is a simple covalent molecule?

A

The chemical molecule (entire structure) which consists of molecules formed when non-metal atoms share and pair valence electrons through covalent bonds (this forms ONE molecule), with weak intermolecular forces holding the other molecules (many others) together within the structure

45
Q

Do simple covalent molecules have high or low melting/boiling points?

A

Low

46
Q

Why do simple covalent molecules have a low melting and boiling points?

A

This is because they have weak intermolecular forces of attraction between the MOLECULES, this means that less energy is required to overcome these forces and break the bonds between the MOLECULES, making it easier for them to melt or boil

Note: For simple covalent molecules it is the WEAK INTERMOLECULAR FORCES that break, not the covalent bonds (never for simple covalent)

47
Q

What is relative molecular mass?

A

It is the sum of the relative atomic masses of all the atoms present in a molecule and is measured in grams per mole (g/mol)

48
Q

How is relative molecular mass calculated?

A

It is calculated by adding together relative atomic masses for all the atoms shown in its chemical formula

49
Q

How does relative molecular mass affect the melting and boiling points of simlpe covalent molecules?

A

A higher relative molecular mass increases the number of molecules and the strength of intermolecular forces, requiring more energy to overcome, which raises the melting and boiling points

50
Q

Do simple covalent molecules conduct electricity? If not, why?

A

No, simple covalent molecuels do not conduct electricity due to them not having any free-moving ions or electrons as molecules are electrically neutral

51
Q

How are covalent bonds held together?

A

Covalent bonds are held together by the electrostatic force of attraction between the positively charged nucleus of the atoms and the negatively charged shared electrons

52
Q

What types of elements are involved in a giant covalent structure?

A

Graphite, graphene, diamond, silicon ONLY THESE

53
Q

What is a giant covalent compound?

A

The chemical compound (entire structure) consisting of many atoms covalently bonded together in a continuous network

54
Q

Why are giant covalent compounds considered one large molecule?

A

They are considered as one large molecule because they consist of atoms bonded by covalent bonds in a continuous network, with no intermolecular forces between them

55
Q

What does volatility mean?

A

How easy a substance evaporates, high = quick and low = slow rate of evaporation

56
Q

State and explain these properties of diamond: Hardness, Melting point, Conductivity, Solubility

A
  • Hardness: Very hard (Each carbon covalently bonded to 4 others)
  • Melting point: Very high (Strong covalent bond)
  • Conductivity: Doesnt conduct (no delocalised electrons)
  • Solubility (strong covalent bonds)
57
Q

State and explain these properties of graphite: Hardness, Melting point, Conductivity, Solubility

A
  • Hardness: Not hard at all so its soft (layers can slide because of weak force between layers)
  • Melting point: Very high (strong covalent bonds)
  • Conductivity: Can conduct electricity (deloclaised electrons between layers)
  • Solubility: Insoluble (strong covalent bonds)
58
Q

State and explain these properties of silica: Hardness, Melting point, Conductivity, Solubility

A
  • Hardness: Hard (strong covalent bonds holding atoms)
  • Melting point: Very high (strong covalent bonds)
  • Conductivity: Doesnt conduct electricity (no deloalised electrons)
  • Solubility: Insoluble (strong covalent bonds)
59
Q

What are some general properties of giant covalent compounds? (melting point, volatility, solubility)

A
  • Melting point: Low
  • Volatility: Very low
  • Solubility: Insoluble
60
Q

What are Allotropes?

A

They are different forms of the same element that exist in the same physical state but have different atomic arrangements and properties

61
Q

Give some examples of allotropes of carbon (4)

A
  • Diamond
  • Graphite
  • Graphene
  • Fullerene
62
Q

What are fullerenes?

A

A molecule made of carbon atoms, bonded into many different shapes with covalent bonds holding the atoms together

Note: They are just a normal molecule, (they are not a definition or whatever) normal just like diamond

63
Q

What is the most well-known fullerene and what is the chemical formula of it?

A

It is buckminsterfullerene with the chemical formula of C60 and it is a simple covalent molecule, NOT giant

64
Q

Name 4 properties of buckminsterfullerene

A
  • High resistancre to stretch
  • 60 protons and 60 electrons
  • Strong covalent bond (property of simple covalent)
  • Weak intermolecular forces (property of simple covalent)
65
Q

Why do giant covalent compounds have a high melting and boiling point?

A

This is because giant covalent compounds have strong covalent bonds between atoms holding the atoms together, this means that it will require more energy to break these covalent bonds as they are extremely strong

66
Q

Do covalent compounds in general usually conduct electricity?

A

No

67
Q

What is a lattice?

A

A repeating regular arrangement of atoms or ions in molecules (this arrangeemnt occurs in crystal structures)

68
Q

What type of lattice do ionic compounds form?

A

Giant ionic lattices (always)

69
Q

What type of lattice do metallic compounds form?

A

Giant metallic lattices (always)

70
Q

What type of lattice do simple covalent compounds form?

A

THEY DO NOT FORM LATTICES

71
Q

What type of lattice do giant covalent compounds form?

A

Giant covalent lattices (always)

72
Q

What is the octet rule?

A

It is a rule that states atoms tend to form bonds in order to achieve a full outer shell of 8 electrons

Note: the octet rule is SPECIFIC to having 8 outer shell electrons ONLY in a covalent bond

73
Q

What is the reason atoms form bonds? (give 2)

A
  • Atoms form bonds in order to achieve a full outer shell, which is either by making a full shell of 8 electrons (for most elements) or 2 electrons (like hydrogen)
  • And also to stabilise the atom by lowering its potential energy
74
Q

What do stick diagrams reperesent?

A

Represents the number of bonds in a molecule (1 stick shows 1 covalent bond)

75
Q

Notes (for stick diagram):

A
  • Each individual atom in the molecule MUST have 8 valence electrons in hte end to stabilize (including telectrons shared from the covalent bond with the other atom)
  • ONLY exception is hydrogen for this rule as it only needs 2 valence electrons to stabilize
  • Covalent bonds can ONLY be formed between 2 or more atoms
  • There can be double bonds which also exist

Year 10 Chemistry (2 decks)

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