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Chemistry > Bonding and Structure > Flashcards

Bonding and Structure Flashcards

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1
Q

what is a cation and anion

A

cation= positive ion
anion= negative ion

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2
Q

what is the perfect ionic model?

A

Ionic compounds that are composed of cations and anions arranged in a lattice

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3
Q

define an ionic bond

A

Electrostatic attraction between anions and cations in a lattice

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4
Q

How does ionic radii change down a group

A

Ionic radii decreases down a group as the number of electron shells increase

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5
Q

define isoelectronic

A

same electronic configuration

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6
Q

how are isoelectronic cations different to isoelectronic anions

A

isoelectronic anions a larger due to having more electrons

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7
Q

properties of ionic solids

A
  • cannot carry charge
    -cannot conduct electricity
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8
Q

properties of ionic liquids

A

-can carry charge
-can conduct electricity

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9
Q

properties of ionic gasses

A

-cannot conduct electricity
-cannot carry charge

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10
Q

how does the strength of ionic bonds affect Mp/Bp

A

Ionic compounds with stronger ionic bonds have a higher Mp/Bp as there is stronger electrostatic attraction between cations and anions

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11
Q

what is the evidence for ions?

A

Green copper chromate solution(aq) —> Cu+ (blue) moves to anion, Cr- (yellow) moves to cation

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12
Q

Define a covalent bond

A

Strong electrostatic attraction between two nuclei and the shared pair of electrons between them. Occurs from the overlap of orbitals

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13
Q

what is a molecule

A

uncharged group of two or more atoms held together

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14
Q

what is dative covalent bond

A

A covalent bond formed when both electrons come from the same atom

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15
Q

What are the 3 types of covalent substances?

A

-giant covalent e.g diamond
-simple covalent e.g Br2
-non-crystalline e.g polymers

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16
Q

Shapes of molecules : BeCl2

A

-Linear
-Bond angle: 180

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17
Q

Shapes of molecules: BCl3

A

-Trigonal planar
-bond angle: 120

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18
Q

Shapes of molecules: CH4

A

-Tetrahedral
-bond angle: 109.5

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19
Q

Shapes of molecules: PCl5

A

-Trigonal Bipyramidal
-bond angle: 120 and 90

20
Q

Shapes of molecules: SF6

A

-Octahedral
-bond angle: 90 and 180

21
Q

Shapes of molecules: H2O

A

-Bent
-bond angle: 104.5

22
Q

What is the theory for the explanation of the shape of molecules?

A

Valance electron shell repulsion theory (VESPR)

23
Q

Define Electronegativity

A

The ability of an atom’s nucleus to attract bonding electrons in a covalent bond

24
Q

how is the bond described in a covalent if the two elements have different electronegativity

A

the bond is polar

25
Q

How does electronegativity change across a period and down a group?

A

-Across a period: electronegativity increases (ionic character also increases)

-Down a group: electronegativity decreases

26
Q

what happens if a molecule has polar bonds but is symmetrical?

A

The dipoles cancel each other out and the molecule is non-polar

27
Q

What are london forces?

A

An intermolecular force that acts between all covalent molecules which strength depends on the number of electrons in a molecule

28
Q

How are london forces formed?

A

Caused by the fleeting attractions and repulsions between the nuclei of an atom and surrounding clouds of electrons (Temporary instantaneous dipoles)

29
Q

What is the effect of larger molecules on London forces?

A

Larger molecules = more electrons = higher polarisability (extent of which electron clouds can be distorted by an electric charge) = greater possibility for temporary induced dipoles

30
Q

What are permanent dipole forces?

A

Occur between the partial “+” of one molecule and the partial “-“ of another molecule. Acts in addition with london forces

31
Q

What are Hydrogen Bonds?

A

Strongest intermolecular force. Occurs between the partial H+ charge on one molecule and that partial X- charge on another molecule.

32
Q

What is the bond angle around the hydrogen atom in a hydrogen bond?

A

180

33
Q

How does strong intermolecular forces affect Mp/Bp?

A

High(er) Mp/Bp

34
Q

Are most ionic compounds soluble in water?

A

Yes because energy is released in the attraction of the ionic compound’s anions and cations to the partially charged oxygen and hydrogen

35
Q

Are Hydrogen-bonded covalent molecules soluble in water?

A

Yes because they can form hydrogen bonds in the water

36
Q

Are covalent molecules with no hydrogen bonding soluble in water?

A

No but are soluble in organic solvents

37
Q

What is metallic bonding?

A

An attraction between the “sea” of delocalised electrons and the positive ions, which are fixed in a lattice

38
Q

Do group 1 metals have a low Mp/Bp and why?

A

Yes because they only have 1 valance electrons for delocalisation and the ions only carry a 1+ charge

39
Q

What does strength of a metallic bond depend on?

A

Strength depends on the number of valance electrons and the size of the metal ion; smaller ionic radii = stronger bond

40
Q

what does the mobility of delocalised electrons allow metals to do?

A

-Carry Charge
-Malleable
-Ductile

41
Q

What are the 3 main types of lattice?

A

-Ionic
-Covalent
-Metallic

42
Q

How are ionic solids arranged in a lattice?

A

The cations and anions are held together by strong electrostatic forces to form an ionic “crystal”

43
Q

How are Covalent lattices arranged?

A

Lattices are joined by strong covalent forces.
The common allotropes:
- Diamond -Each carbon has 4 sigma bonds forming a tetrahedral structure
-Graphite -Each carbon bonded to 3 other carbons, 1 delocalised electron that can carry charge. Forms layers of hexagonal rings. Layers held by weak London forces

44
Q

What forces acts between Simple covalent substances?

A

Weak intermolecular forces

45
Q

What state do simple covalent molecules tend to be at room temperature?

A

Liquid or gas depending in the size of the covalent molecule which affects the strength of London Forces and therefore Mp/Bp

46
Q

What forces act between polar molecules?

A

London forces + Permanent dipole forces

47
Q

What bonds occur between organic acids and alcohols?

A

London Forces + Hydrogen bonds

Chemistry (4 decks)

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