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Y10 Chem 2024 > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

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1
Q

Isotopes

A

same number of protons, different number of neutrons (and therefore different atomic mass number)

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2
Q

Atom

A

Atoms are composed of electrons and a nucleus. The nucleus contains protons and neutrons.

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3
Q

Element

A

When a substance contains only one type of atom, it is called an element.

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4
Q

Ions

A

an atom or molecule with a charge due to the loss or gain of one or more electrons

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5
Q

Electronegativity

A

a measure of an atom’s ability to attract shared electrons

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6
Q

Periods

A

horizontal rows on the periodic table (number of electron shells in an atom of that element).

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7
Q

Groups

A

vertical columns on the periodic table (number of valence electrons in the valence/outer electron shell - exception transition metals).

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8
Q

Atomic Radii

A

the total distance from an atom’s nucleus to the outermost orbital of electron (decreases down a period and increases down a group)

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9
Q

Ionic Bonding

A

The strong electrostatic force of attraction between positively and negatively charged ions.

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10
Q

Monatomic ions

A

Ion formed from a single atom i.e Cl–> Cl-

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11
Q

Polyatomic ions

A

A group of atoms covalently bonded together, but the group of atoms as a whole has a charge.

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12
Q

Ionic Property: Hardness

A

Structure: Giant Ionic Lattice
Bonding: Strong electrostatic force of attraction between oppositely charged ions which requires a lot of force to break

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13
Q

Ionic Property: High MP/BP

A

Structure: Giant Ionic Lattice
Bonding: Strong electrostatic force of attraction between oppositely charged ions which requires a lot of energy to break

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14
Q

Ionic Property: Brittle

A

Structure: Giant Ionic Lattice
Bonding: Lattice arrangement of ions that, when a strong enough force is applied, the lattice may shift and like charges align and repel. This breaks the lattice.

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15
Q

Ionic Property: Conductivity

A

Structure: Giant Ionic Lattice
Bonding: To conduct electricity, there needs to be a flow of charged particles (ions). As a solid, ions are not free to move and carry charge whereas as a liquid/molten the ions are free to move and carry charge.

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16
Q

Chemical Equations

A

Format: REACTANTS –> PRODUCTS

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17
Q

Aqueous state symbol

A

Dissolved in water (Aq)

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18
Q

Solid state symbol

A

(s)

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19
Q

Liquid state symbol

A

(l)

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20
Q

Gas state symbol

A

(g)

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21
Q

Sulfate ion

A

SO4 (2-)

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22
Q

Carbonate ion

A

CO3 (2-)

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23
Q

Alloy

A

Mixtures of two or more metal elements

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24
Q

Common properties of metals

A

Melting Points
Boiling Points
Lustre
Malleability
Ductile
Heat conductivity
Electrical conductivity

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25
Q

Metallic bonding

A

Metallic bonding is the electrostatic attraction between cations and their delocalized valence electrons.

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26
Q

Metallic structure

A

Giant metallic lattice

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27
Q

Metallic Property: High MP/BP

A

Structure: Giant metallic lattice
Bonding: strong electrostatic forces of attraction between cations and the sea of delocalized electrons which require a lot of energy to break

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28
Q

Metallic Property: Lustre

A

Structure: Giant metallic lattice
Bonding: a sea of delocalized electrons exist within the lattice that are able to reflect light

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29
Q

What does malleable mean?

A

Able to be changed shape (into thin sheets)

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30
Q

Metallic Property: Malleable & Ductile

A

Structure: Giant metallic lattice
Bonding: strong electrostatic forces of attraction between cations and the sea of delocalized electrons which means the shape can be changed without the forces being broken

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31
Q

What does ductile mean?

A

Ability to be shaped into thin wires

32
Q

Metallic property: Heat conductivity

A

Structure: Giant metallic lattice
Bonding: Kinetic energy of cations (vibrations) and electrons (movement) is passed efficiently through the metal

33
Q

Metallic property: Electrical conductivity

A

Structure: Giant metallic lattice
Bonding: Delocalized valence electrons are free to move and carry a charge.

34
Q

Displacement reaction

A

a more reactive element takes the place of a less reactive element in a salt.

35
Q

METAL + DILUTE ACID –>

A

SALT + HYDROGEN

36
Q

METAL + OXYGEN –>

A

METAL OXIDE

37
Q

METAL + WATER –>

A

METAL HYDROXIDE + HYDROGEN

38
Q

METAL + STEAM –>

A

METAL OXIDE + HYDROGEN

39
Q

Electronegativity

A

The tendency in which atoms or molecules pull electrons towards itself.

40
Q

Polar

A

Uneven distribution of electrons

41
Q

Giant Covalent Lattice

A

3-dimensional structure arising from atoms forming many covalent bonds.

42
Q

Examples of giant covalent lattice structures

A

Graphite and diamond

43
Q

Giant Cov. Property: Hardness (Diamond)

A

Structure: Giant Covalent Lattice
Bonding: Many covalent bonds within the structure which can withstand significant force

44
Q

Giant Cov. Property: Softness (Graphite)

A

Structure: Giant Covalent Lattice
Bonding: Layers of carbon sheets with delocalised electrons between the layers. These sheets can slide over each other easily.

45
Q

Giant Cov. Property: Electrical Conductivity (Graphite)

A

Structure: Giant Covalent Lattice
Bonding: Layers of carbon sheets with delocalised electrons between the layers. These delocalised electrons can move and carry charge.

46
Q

Giant Cov. Property: Conductivity (Graphite)

A

Structure: Giant Covalent Lattice
Bonding: Diamond does not contain any free moving charged particles and so cannot conduct electricity.

47
Q

Intramolecular

A

Forces within molecules/compounds.

48
Q

Examples of intramolecular forces

A
  • Ionic Bonding
  • Metallic Bonding
  • Covalent Bonding
49
Q

Intermolecular

A

forces found between simple covalent molecules.

50
Q

Examples of intermolecular forces

A
  • Dispersion forces
  • Dipole-dipole forces
  • Hydrogen bonds
51
Q

Dispersion forces (temporary)

A

Occur between all molecules and atoms due to the constant movement of electrons

52
Q

Dipole-Dipole forces (permanent)

A

Attraction between polar simple covalent molecules.

53
Q

Hydrogen bond

A

“extra-strong” dipole-dipole attraction between H-NOF of one molecule and NOF of a neighbouring molecule

54
Q

Solute

A

the substance being dissolved

55
Q

Solvent

A

is the primary component of the solution. It does the dissolving.

56
Q

Solution

A

an evenly distributed mixture of atoms, molecules and/or ions including a liquid solvent and one or more solutes.

57
Q

Precipitate

A

is an insoluble salt formed from two aqueous reagents.

58
Q

Spectator Ions

A

ions not involved in a chemical reaction that remain in solution

59
Q

What does the term ‘giant’ mean when talking about a structure?

A

An unlimited/undefined number of particles in the structure.

60
Q

What does the term ‘lattice’ mean when talking about a structure?

A

A regular, repeating 3-dimensional arrangement

61
Q

Covalent Bonding

A

The electrostatic force of attraction between two atomic nuclei and a shared pair of valence electrons between those atoms

62
Q

Covalent Molecular Property: Low MP/BP

A

Structure: Simple covalent molecular
Bonding: Weak intermolecular forces exist between molecules which do not require a lot of energy to overcome

63
Q

Covalent Molecular Property: Does not conduct electricity

A

Structure: Simple covalent molecular

64
Q

Test for metal cations

A

Flame test

65
Q

Ca2+ ion flame colour

A

Brick Red

66
Q

K+ ion flame colour

A

Purple

67
Q

Na+ ion flame colour

A

Orange

68
Q

Li+ ion flame colour

A

Red

69
Q

Describe the test for ammonia

A

add 3 drops of dilute sodium hydroxide solution
gently heat
if NH4+ is present - characteristic choking smell produced. The ammonia fumes turn damp red litmus paper or damp universal indicator paper from red to blue.

70
Q

Describe the test for carbonate ions

A

add 3 drops of dilute hydrochloric acid
bubble gas through limewater
if CO32- present, limewater turns cloudy

71
Q

Describe the test for sulfate ions

A

add 3 drops of dilute hydrochloric acid
add 3-4 drops of barium chloride solution
if SO42- present a white precipitate forms

72
Q

Describe the test for halide ions

A

Add 3 drops of dilute nitric acid
then add 3-4 drops of silver nitrate solution

73
Q

Colour change when chloride ions are present

A

White

74
Q

Colour change when bromide ions are present

A

Cream

75
Q

Colour change when iodide ions are present

A

Yellow

Y10 Chem 2024 (5 decks)

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