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chem yr 10 > 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 composition

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

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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 when chemically combined with another element

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6
Q

Core Charge

A

A measure of the attractive force felt by the valence electrons towards the nucleus.

protons - # inner electrons = core charge

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7
Q

What does it mean by no two electrons can occupy the same state?

A

No two electrons can be in the same ‘place’ at the same time with the same magnetic spin and energy

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8
Q

Atomic Radii

A

the total distance from an atom’s nucleus to the outermost orbital of electron

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9
Q

What is atomic radius influenced by?

A
  • Number of occupied shells
  • Core Charge
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10
Q

Why does atomic radius decrease down a period and increase down a group?

A

Decreases down a period: Occupied energy levels are constant but core charge increases

Increases down a group:
Occupied energy levels increases but core charge is same

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11
Q

Electron shielding

A

Repulsive force exerted by inner shell electrons on outer shell electrons, forcing them away from the nucleus

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12
Q

Ionic Bonding

A

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

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13
Q

Monatomic ions

A

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

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14
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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15
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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16
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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17
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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18
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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19
Q

Chemical Equations

A

Format: REACTANTS –> PRODUCTS

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20
Q

Aqueous state symbol

A

Dissolved in water (Aq)

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21
Q

Solid state symbol

A

(s)

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22
Q

Liquid state symbol

A

(l)

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23
Q

Gas state symbol

A

(g)

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24
Q

Sulfate ion

A

SO4 (2-)

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25
Carbonate ion
CO3 (2-)
26
Alloy
Mixtures of two or more metal elements
27
Common properties of metals
Melting Points Boiling Points Lustre Malleability Ductile Heat conductivity Electrical conductivity
28
Metallic bonding
Metallic bonding is the electrostatic attraction between cations and their delocalized valence electrons.
29
Metallic structure
Giant metallic lattice
30
Metallic Property: High MP/BP
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
31
Metallic Property: Lustre
Structure: Giant metallic lattice Bonding: a sea of delocalized electrons exist within the lattice that are able to reflect light
32
What does malleable mean?
Able to be changed shape (into thin sheets)
33
Metallic Property: Malleable & Ductile
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
34
What does ductile mean?
Ability to be shaped into thin wires
35
Metallic property: Heat conductivity
Structure: Giant metallic lattice Bonding: Kinetic energy of cations (vibrations) and electrons (movement) is passed efficiently through the metal
36
Metallic property: Electrical conductivity
Structure: Giant metallic lattice Bonding: Delocalized valence electrons are free to move and carry a charge.
37
Displacement reaction
a more reactive element takes the place of a less reactive element in a salt.
38
METAL + DILUTE ACID -->
SALT + HYDROGEN
39
METAL + OXYGEN -->
METAL OXIDE
40
METAL + WATER -->
METAL HYDROXIDE + HYDROGEN
41
METAL + STEAM -->
METAL OXIDE + HYDROGEN
42
Polar
Uneven distribution of charge
43
Giant Covalent Lattice
3-dimensional structure arising from atoms forming many covalent bonds.
44
Examples of giant covalent lattice structures
Graphite and diamond
45
Giant Cov. Property: Hardness (Diamond)
Structure: Giant Covalent Lattice Bonding: Many covalent bonds within the structure which can withstand significant force
46
Giant Cov. Property: Softness (Graphite)
Structure: Giant Covalent Lattice Bonding: Layers of carbon sheets with delocalised electrons between the layers. These sheets can slide over each other easily.
47
Giant Cov. Property: Electrical Conductivity (Graphite)
Structure: Giant Covalent Lattice Bonding: Layers of carbon sheets with delocalised electrons between the layers. These delocalised electrons can move and carry charge.
48
Giant Cov. Property: Conductivity (Graphite)
Structure: Giant Covalent Lattice Bonding: Diamond does not contain any free moving charged particles and so cannot conduct electricity.
49
Intramolecular
Forces within molecules/compounds.
50
Examples of intramolecular forces
- Ionic Bonding - Metallic Bonding - Covalent Bonding
51
Intermolecular
forces found between simple covalent molecules.
52
Examples of intermolecular forces
- Dispersion forces - Dipole-dipole forces - Hydrogen bonds
53
Dispersion forces
Attraction between temporary, instantaneous dipoles.
54
Dipole-Dipole forces (permanent)
Attraction between polar simple covalent molecules.
55
Hydrogen bond
dipole-dipole attraction between H-NOF of one molecule and NOF of a neighbouring molecule
56
Solute
the substance being dissolved
57
Solvent
is the primary component of the solution. It does the dissolving.
58
Solution
an evenly distributed mixture of atoms, molecules and/or ions including a liquid solvent and one or more solutes.
59
Precipitate
is an insoluble salt formed from two aqueous reagents.
60
What is a net ionic equation?
Equ. of precipitation reaction without spectator ions
61
Spectator Ions
ions not involved in a chemical reaction that remain in solution
62
What does the term 'giant' mean when talking about a structure?
An unlimited/undefined number of particles in the structure.
63
What does the term 'lattice' mean when talking about a structure?
A regular, repeating 3-dimensional arrangement
64
Covalent Bonding
The electrostatic force of attraction between two atomic nuclei and a shared pair of valence electrons between those atoms
65
Covalent Bond Property: Localised and Directional
Localised: held in place by positive nuclei Directional: well-defined place
66
Covalent Molecular Property: Low MP/BP
Structure: Simple covalent molecular Bonding: Weak intermolecular forces exist between molecules which do not require a lot of energy to overcome
67
Giant Covalent Lattice Property: High MP/BP
Bonding: Strong intermolecular forces exist between molecules which require a lot of energy to overcome
68
Covalent Molecular Property: Does not conduct electricity
Structure: No charged particles free to move Bonding: Localised electrons held in place (except graphite)
69
Covalent Molecular Property: Hard
Bonds are strong so they resist indentation
70
Describe graphite structure
Carbon atoms covalently bonded to 3 others, forming layers. 4th electron is delocalised and moves between layers. Weak dispersion forces between layers: soft Delocalised 4th electron: can conduct electricity
71
Test for metal cations
Flame test
72
Ca2+ ion flame colour
Brick Red
73
K+ ion flame colour
Purple
74
Na+ ion flame colour
Orange
75
Li+ ion flame colour
Red
76
Describe the test for ammonia
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.
77
Describe the test for carbonate ions
add 3 drops of dilute hydrochloric acid bubble gas through limewater if CO32- present, limewater turns cloudy
78
Describe the test for sulfate ions
add 3 drops of dilute hydrochloric acid add 3-4 drops of barium chloride solution if SO42- present a white precipitate forms
79
Describe the test for halide ions
Add 3 drops of dilute nitric acid then add 3-4 drops of silver nitrate solution
80
Colour change when chloride ions are present
White
81
Colour change when bromide ions are present
Cream
82
Colour change when iodide ions are present
Yellow
83
Possible molecule shapes for molecule with two electron groups
Linear (no lone pair) Diatomic (1 lone pair)
84
Possible molecule shapes for molecule with three electron groups
Trigonal Planar (0) Bent (1) Diatomic (2)
85
Possible molecule shapes for molecule with four electron groups
Tetrahedral (0) Trigonal Planar (1) Bent (2) Diatomic (3)

chem yr 10 (5 decks)

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