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IB Chemistry > Structure 2.1/2 The Ionic and Covalent Model > Flashcards

Structure 2.1/2 The Ionic and Covalent Model Flashcards

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1
Q

What are ions?

A

Atoms or groups of atoms with an overall charge

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2
Q

How are ions formed?

A

Transfer of electrons from one atom to another, which results in both atoms having a full outer shell

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3
Q

What do metal atoms generally form in terms of ions?

A

Cations: positively charged ion

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4
Q

What do non-metal atoms generally form in terms of ions?

A

Anion: negatively charged ion

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5
Q

What are ionic compounds?

A

Compounds made up of a combination of cations and anions

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6
Q

What is ionic bonding?

A

Electrostatic attraction between ions of opposite charges

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7
Q

What are transition elements?

A

Elements whose atoms have incomplete d-subshells or who can give rise to cations with incomplete d subshells

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8
Q

What does isoelectronic mean?

A

Same amount of electrons

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9
Q

Which monatomic ions tend to possess the electron configuration of a noble gas?

A

Main group elements (not Group 14)

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10
Q

What is a polyatomic ion?

A

Overall charged unit of groups of joined atoms

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11
Q

What does the term ‘protonated’ mean?

A

Adding of a hydrogen ion (essentially just a proton)

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12
Q

What does the term deprotonated mean?

A

Removal of a hydrogen ion (essentially just a proton)

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13
Q

What is the empirical formulae?

A

Simplest ratio of atoms of each elements present in that compound

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14
Q

What form is the formula of an ionic compound written in?

A

Empirical formula

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15
Q

How to write an ionic compound?

A
  1. Name of positive ion (cation) first
  2. Include roman numerals if cation is a transition element
  3. Wirte name of anion (monatomic = ends with ‘ide’)
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16
Q

What do Roman numerals indicate on a transition metal?

A

Oxidation state (similar to charge on an ion) of metallic elements

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17
Q

What is an ionic lattice?

A

Regular, repeating 3-dimensional arrangement of cations and anions

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18
Q

How do ions arrange themselves in an ionic compound?

A

In the most stable configuration. Oppositely charged ions are as close together as possible. Ions of the same charge are as far apart as possible

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19
Q

What are the properties of ionic compounds?

A

Crystalline
Low volatilities
High melting and boiling points
Conduct electricity while molten or in aqueous solution (not when solid)
Some are soluble in water
Hard
Brittle

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20
Q

Why are ionic compounds crystalline?

A

Structure of lattice

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21
Q

What is the ionic radius?

A

In a crystalline ionic compound, it is the distance from the nucleus to the valence shell

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22
Q

What happens to the radius of an atom when it becomes a cation?

A

Reduces.
Loses a shell

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23
Q

What happens to the radius of an atom when it becomes an anion?

A

Enlarges.
Repel other electrons + swell atoms

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24
Q

What influences the structure of the ionic lattice?

A

Size of ionic radii
Charge of ions

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25
What is volatility?
Measure of how readily a substance evaporates below its boiling point
26
Why do ionic compounds have high melting and boiling points?
Electrostatic attraction between charges is very strong. Large amounts of thermal energy are requried to separate ions
27
What is lattice enthalpy?
Energy needed to separate one mole of a solid ionic compound into gaseous ions under standard conditions
28
What is the formula for the lattice enthalpy of MgCl2?
MgCl2(s) -> Mg2+(g) + 2Cl-(g)
29
What units are lattice enthalpies measured in?
kJ / mol
30
What are endothermic reactions?
Processes that require energy
31
What are exothermic reactions?
processes that release energy
32
What type of reaction is a lattice enthalpy?
Endothermic
33
What is the relationship between ionic charge and lattice enthalpy?
Greater charge on ion = stronger electrostatic attraction = higher lattice enthalpy
34
What is the relationship between ionic radii and lattice enthalpy?
Larger ionic radii = greater separation of charges = weaker the electrostatic attraction = lower lattice enthalpy
35
What is relationship between attractive force and theoretical lattice enthalpy?
Attractive force ∝ theoretical lattice enthalpy ∝ (charge on cation x charge on anion) / sum of ionic radii
36
What is required for a substance to conduct electricity?
Free moving, charged particles
37
Can solid ionic compounds conduct electricity?
No. the ions are held rigidly in place within the lattice and are not free to move.
38
Can molten/aqeuous solutions conduct electricity?
Yes. Ions are free to move towards electrodes of opposite charge
39
What is the solubility of a substance?
Maximum amount of that substance that can be dissolved in a given quantity of solvent at a given temperature
40
What is a saturated solution?
A solution where no more solute can be dissolved at that temperature
41
In an insoluble substance, the energy required to separate the ions is much greater than?
The energy released when the ions become hydrated
42
What happens when a soluble compound dissolves in water?
Ionic bonds within solid lattice are broken Hydrogen bonds between adjacent water molecules are broken ion-dipole bonds are formed between ions adn water molecules Ions become hydrated (solvated by water molecules)
43
If two aqeuous solutions are together and form a precipitate, what has been formed?
An insoluble solution
44
Why are ionic compounds hard?
Strong electrostatic attraction between cations and anions causes crystals to resist change in shape + be hard
45
Why are ionic compounds brittle?
IF sufficient force is applied to crystalline lattice - rows of ions will move relative to one another - ions of like charges will become adjacent - adjacent ions of like charge will repel each other (causing lattice to shatter)
46
What are covalent substances?
Formed when non-metallic elements join together
47
What are some traits of colavent substances?
Solids/liquids/gases at room temperature Can have low melting/boiling points Generally poor conductors of electricity and heat
48
What is a covalent bond?
A shared pair of electrons
49
How do non-metals bond together?
sharing one or more pairs of electrons
50
What bonds two non-metals together?
Electrostatic attraction of two nuclei towards shared pair of electrons
51
What happens if two atom nuclei are too far apart?
no attraction
52
What does the optimal bond length involve?
Maximising attraction between the two positive nuclei to the shared pair of negative electrons while minimising the repulsion between two positive nuclei
53
What can covalent bonds form between?
discrete molecules large molecules covalent networks
54
What are discrete covalent molecules?
small groups of atoms held together by strong covalent bonds
55
What do covalent bonds between large numbers of atoms form?
Large molecules such as polymers, plastics, fullerenes
56
What do covalent bonds between an infinite number of atoms form?
Covalent networks such as graphite, diamond, silicon, etc
57
What is the octet rule?
Tendency of atoms to achieve a full valence shell with a total of 8 electrons
58
What do Lewis formulas show?
All valence electrons - bonding pairs - non-bonding pairs
59
How to draw Lewis formulas of molecules and ions?
1. Add up total number of valence electrons (including charges) 2. Write atoms in order bonded - non-metal atom (with the lowest electronegativity = most top right of table) that forms most bonds will usually be central atom 3. Place single covalent bonds betweeen atoms 4. Place non-bonding electrons to the non-central atoms so that each has an octet of electrons 5. Place any remaining on central atom 6. Use lone pairs on non-central atoms to form double/triple bonds to ensure the central atom has an octet 7. Draw square brackets around Lewis formula and write overall charger outside brackets at top right corner if polyatomic
60
How to find element with lowest electronegativity via a periodic table?
Most to right
61
What is the relationship between bond strength and amount of bonds?
More bonds (i.e. triple covalent bond) = stronger
62
What is the relationship between bond strength and amount of bonds?
More bonds = stronger bond
63
What does VSEPR stand for?
Valence Shell Electron Pair Repulsion
64
What does the VSEPR model enable?
The shape of the molecules to be predited from the repulsion of electron domains around a central atom
65
What is an electron domain?
region where electrons are likely to be found
66
What can each electron domain be occupied by?
A single electron Lone pair Single bond Double bond Triple bond
67
How are electron domains orientated?
As far away as possible from each other in 3D space
68
What are the three electron domain geometry options?
Linear Trigonal planar Tetrahedral
69
What are thre five molecular geometry options?
Linear V-shaped Trigonal planar Trigonal pyramidal Tetrahedral
70
What is the electron domain geometry of a central atom surrounded by 4 occupied electron domains?
Tetrahedral
71
What is the electron domain geometry of a central atom surrounded by 3 occupied electron domains?
Trigonal planar
72
What is the electron domain geometry of a central atom surrounded by 2 occupied electron domains?
Linear
73
What is the molecular geometry of a central atom surrounded by 4 occupied electron domains and 0 lone pairs?
Tetrahedral 109.5 degree bond angle
74
What is the molecular geometry of a central atom surrounded by 4 occupied electron domains and 1 lone pairs?
Trigonal pyramidal 107 degree bond angle
75
What is the molecular geometry of a central atom surrounded by 4 occupied electron domains and 2 lone pairs?
Bent 105 degree
76
What is the molecular geometry of a central atom surrounded by 4 occupied electron domains and 3 lone pairs?
Linear
77
What is the molecular geometry of a central atom surrounded by 3 occupied electron domains and 0 lone pairs?
trigonal planar
78
What is the molecular geometry of a central atom surrounded by 3 occupied electron domains and 1 lone pairs?
V-shaped
79
What is the molecular geometry of a central atom surrounded by 3 occupied electron domains and 2 lone pairs?
Linear
80
What is the molecular geometry of a central atom surrounded by 2 occupied electron domains and 0 lone pairs?
Linear 180 degrees
81
What is the molecular geometry of a central atom surrounded by 2 occupied electron domains and 1 lone pairs?
Linear
82
What is the molecular formula?
The actual number of atoms of each element present in a covalent molecular substance
83
What is the order of repulsion in terms of bonding pairs and lone pairs?
Least repulsed: bonding pair + bonding pair Middle repulsed: bonding pair + lone pair Most repulsed: lone pair + lone pair
84
What is a coordination bond?
Covalent bond in which both the electrons of the shared pair originate from the same atom?
85
How is ammonium formed?
NH3(aq) + H+(aq) -> NH4+ (aq)
86
How to know if a coordinate bond has occured?
One atom will have formed more bonds that usual

IB Chemistry (11 decks)

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