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Y10 Chem 2025 > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

(75 cards)

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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
Metallic bonding
Metallic bonding is the electrostatic attraction between cations and their delocalized valence electrons.
26
Metallic structure
Giant metallic lattice
27
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
28
Metallic Property: Lustre
Structure: Giant metallic lattice Bonding: a sea of delocalized electrons exist within the lattice that are able to reflect light
29
What does malleable mean?
Able to be changed shape (into thin sheets)
30
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
31
What does ductile mean?
Ability to be shaped into thin wires
32
Metallic property: Heat conductivity
Structure: Giant metallic lattice Bonding: Kinetic energy of cations (vibrations) and electrons (movement) is passed efficiently through the metal
33
Metallic property: Electrical conductivity
Structure: Giant metallic lattice Bonding: Delocalized valence electrons are free to move and carry a charge.
34
Displacement reaction
a more reactive element takes the place of a less reactive element in a salt.
35
METAL + DILUTE ACID -->
SALT + HYDROGEN
36
METAL + OXYGEN -->
METAL OXIDE
37
METAL + WATER -->
METAL HYDROXIDE + HYDROGEN
38
METAL + STEAM -->
METAL OXIDE + HYDROGEN
39
Electronegativity
The tendency in which atoms or molecules pull electrons towards itself.
40
Polar
Uneven distribution of electrons
41
Giant Covalent Lattice
3-dimensional structure arising from atoms forming many covalent bonds.
42
Examples of giant covalent lattice structures
Graphite and diamond
43
Giant Cov. Property: Hardness (Diamond)
Structure: Giant Covalent Lattice Bonding: Many covalent bonds within the structure which can withstand significant force
44
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.
45
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.
46
Giant Cov. Property: Conductivity (Graphite)
Structure: Giant Covalent Lattice Bonding: Diamond does not contain any free moving charged particles and so cannot conduct electricity.
47
Intramolecular
Forces within molecules/compounds.
48
Examples of intramolecular forces
- Ionic Bonding - Metallic Bonding - Covalent Bonding
49
Intermolecular
forces found between simple covalent molecules.
50
Examples of intermolecular forces
- Dispersion forces - Dipole-dipole forces - Hydrogen bonds
51
Dispersion forces (temporary)
Occur between all molecules and atoms due to the constant movement of electrons
52
Dipole-Dipole forces (permanent)
Attraction between polar simple covalent molecules.
53
Hydrogen bond
“extra-strong” dipole-dipole attraction between H-NOF of one molecule and NOF of a neighbouring molecule
54
Solute
the substance being dissolved
55
Solvent
is the primary component of the solution. It does the dissolving.
56
Solution
an evenly distributed mixture of atoms, molecules and/or ions including a liquid solvent and one or more solutes.
57
Precipitate
is an insoluble salt formed from two aqueous reagents.
58
Spectator Ions
ions not involved in a chemical reaction that remain in solution
59
What does the term 'giant' mean when talking about a structure?
An unlimited/undefined number of particles in the structure.
60
What does the term 'lattice' mean when talking about a structure?
A regular, repeating 3-dimensional arrangement
61
Covalent Bonding
The electrostatic force of attraction between two atomic nuclei and a shared pair of valence electrons between those atoms
62
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
63
Covalent Molecular Property: Does not conduct electricity
Structure: Simple covalent molecular
64
Test for metal cations
Flame test
65
Ca2+ ion flame colour
Brick Red
66
K+ ion flame colour
Purple
67
Na+ ion flame colour
Orange
68
Li+ ion flame colour
Red
69
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.
70
Describe the test for carbonate ions
add 3 drops of dilute hydrochloric acid bubble gas through limewater if CO32- present, limewater turns cloudy
71
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
72
Describe the test for halide ions
Add 3 drops of dilute nitric acid then add 3-4 drops of silver nitrate solution
73
Colour change when chloride ions are present
White
74
Colour change when bromide ions are present
Cream
75
Colour change when iodide ions are present
Yellow

Y10 Chem 2025 (5 decks)

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