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Chemistry LC 2022 > 5. Chemical Bonding > Flashcards

5. Chemical Bonding Flashcards

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1
Q

Compund

A

A substance made of two or more elements chemicals combined

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2
Q

Octet rule

A

When bonding occurs, atoms tend to reach an electron arrangement with 8 electrons in the outermost energy level.

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3
Q

What are the exceptions to the octet rule?

A

Transition metals

Hydrogen, Lithium & Beryllium (2)

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4
Q

Ion

A

A charged atom or group of atoms.

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5
Q

Cations

A

Positive ions

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6
Q

Anions

A

Negative ions

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7
Q

Ionic bond , eg

A

The force of attraction between oppositely charged ions in a compound. Ionic bonds are always formed by the complete transfer of electrons from one atom to another.
Eg NaCl

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8
Q

What is the name of the three dimensional structure in which ions are encased?

A

Crystal lattice

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9
Q

3 characteristics of transition metals

A
  • variable valency
  • coloured compounds
  • catalysts
    VCC
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10
Q

What elements included in the d block are not actually transition metals?

A

Scandium and Zinc

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11
Q

Transition metal

A

One that forms at least one ion with a partially filled d sublevel.

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12
Q

Molecule

A

A group of atoms joined together. It is the smallest particle of an element or compound that can exist independently.

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13
Q

Valency

A

Valency of an element is defined as the no. of atoms of hydrogen or any other monovalent element with which each atom of the element combines.

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14
Q

Sigma bond

A

A sigma bond is formed by the head on overlap of two orbitals.
(Single bonds) eg H2

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15
Q

Pi bond

A

Pi bonds are formed by the sideways overlap of p orbitals.

Eg O2

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16
Q

What type of bonds make up a single bond?

A

1 sigma bond

17
Q

What type of bonds make up a double bond?

A

1 sigma

1 pi bond

18
Q

What type of bonds make up triple bonds?

A

1 sigma

2 pi

19
Q

Which are stronger, sigma or pi bonds?

A

Sigma ; as there is more overlapping of orbitals in sigma bonds
Therefore O=O is not twice as strong as O-O.

20
Q

VSEPR

A

Valence Shell Electron Pair Repulsion

Electron pairs repel each other and arrange themselves in space so they can be as far apart as possible

21
Q

Angle of Triangular Planar

A

120

22
Q

Angle of linear

A

180

23
Q

Angle of pyramidal

A

107

24
Q

Angle of V shaped

A

104.5

25
Q

Angle of Tetrahedral

A

109.5

26
Q

Electronegativity

A

The relative attraction that an atom in a molecule has for the shared pair(s) of electrons in a covalent bond.

27
Q

Polar covalent bond

A

A bond in which there is unequal sharing of the pair(s) of electrons. This causes one end of the bond to be slightly negative and the other end slightly positive.

28
Q

Pure covalent

A

Equal sharing

29
Q

Exception to polar covalent bonds

A

Symmetrical molecules eg CO2 where the center of the negative charges coincide with that of the positive charges .

30
Q

Demonstrate polarity of water molecule

A

A charged plastic rod will always attract the water stream, whether negative or positive charged. Bc water molecules spin so that the neg/pod charge are attracted to rod.

31
Q

Predicting type of bonding based one electronegativity values

A

0- non polar (pure covalent)
0-0.4 negligible polar covalent
0.4-1.7 polar covalent
1.7+ ionic

32
Q

Intramolecular bonding

A

Bonding that takes place within the molecule ie it holds the atoms together. Eg Covalent, polar covalent

33
Q

Intermolecular forces

A

The forces of attraction that exist between molecules. Eg Van der Waals, dipole-dipole, hydrogen bonds.

34
Q

Van der Waals forces

A

Weak attractive forces between molecules resulting from the formation of temporary dipoles. They are the only forces of attraction between non-polar molecules
Eg. H2

35
Q

Dipole-dipole forces

A

The forces of attraction between the negative pole of one polar molecule and the positive pole of another polar molecule. Eg HCl

36
Q

Hydrogen Bonds

A

Particular types of dipole-dipole attractions between molecules in which hydrogen atoms are bonded with nitrogen, oxygen or fluorine.
NOF

Chemistry LC 2022 (7 decks)

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