Topic 4 - Bonding & Structure

Question 1

Hybridization

Answer 1

The process of mixing atomic orbitals to form new hybrid orbitals that can be used for bonding in molecules

Question 2

Sigma Bonds

Answer 2

The overlapping of hybrid orbitals across the axis.

Question 3

sp Hybridization

Answer 3

1 s orbital and 1 p orbital mix to form 2 equivalent sp hybrid orbitals, typically seen in linear molecules (2 bonding sites).

Question 4

sp2 Hybridization

Answer 4

1 s orbital and 2 p orbitals resulting in 3 sp2 hybrid orbitals, commonly found in trigonal planar structures (3 bonding sites).

Question 5

sp3 Hybridization

Answer 5

1 s orbital and 3 p orbitals combine to form 4 equivalent sp3 hybrid orbitals, characteristic of tetrahedral geometry (4 bonding sites).

Question 6

dsp3 Hybridization

Answer 6

1 s orbital and 3 p orbital and 1 d orbital resulting in 5 dsp3 orbitals, found in trigonal bipyramidal structures (5 bonding sites).

Question 7

d2sp3 Hybridization

Answer 7

1 s orbital and 3 p orbitals and 2 d orbitals combine to form 6 equivalent d2sp3 hybrid orbitals, found in octahedral structures (6 bonding sites).

Question 8

Orbital Mixing

Answer 8

atomic orbitals combine to create new orbitals with different shapes and energies.

Question 9

Tetrahedral Geometry

Answer 9

The central atom is bonded to 4 other atoms, bond angles of approximately 109.5 degrees, typical of sp3 hybridization.

Question 10

Trigonal Planar Geometry

Answer 10

The central atom is bonded to 3 other atoms, with bond angles of 120 degrees, associated with sp2 hybridization.

Question 11

Elements happy with an incomplete octet

Answer 11

Boron and Beryllium because they are electron deficient they react with molecules that have lone pairs of electrons like H2O + NH3, they are also Lewis Acids = electron seeking.

Question 12

Resonance Structures

Answer 12

different ways of drawing the same molecule, showing the delocalization of electrons across multiple positions, which contributes to the overall stability of the molecule.

Question 13

Lewis Structures

Answer 13

Diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist, helping to visualize the arrangement of electrons

Question 14

Delocalized Electrons

Answer 14

electrons that are not associated with a single atom or bond but are spread over several atoms, contributing to the stability and reactivity of molecules.

Question 15

Double Bond

Answer 15

Formed from the overlapping of a hybridized and overlapping of an unhybridized orbital. 4 electrons, 2 pairs

Question 16

Bond length

Answer 16

distance between the nuclei of two bonded atoms, which can vary depending on the type of bond
Single > Double > Triple

Question 17

Bond Strength

Answer 17

Refers to the energy required to break a bond between two atoms; stronger bonds have shorter lengths and higher bond orders

Question 18

Metallic bonding

Answer 18

A type of chemical bonding that occurs between metal atoms, characterized by the sharing of free electrons among a lattice of cations

Question 19

Delocalized Electrons contribute to characteristics such as..

Answer 19

Malleability, Ductility, Conductivity of heat and energy, shine/luster

Question 20

Cation Size/# of delocalized Electrons contribute to….

Answer 20

The smaller the cation and as the number of delocalized Electrons increases, the stronger the metallic bond.
Mg+2 is stronger than Na+ because it is smaller and has more delocalized electrons

Question 21

Transition metals

Answer 21

Found in the d-block of the periods. Greater delocalization of electrons and stronger metallic bonding.

Question 22

Strength of Metallic bonds

Answer 22

Increases with the number of delocalized electrons and size of cations; smaller cations and more delocalized electrons increase bond strength.

Question 23

Pi orbitals

Answer 23

The overlapping of unhybrid orbitals above and below the axis.

Question 24

Triple bonds

Answer 24

formed from the overlapping of hybridized and two unhybridized orbitals

Question 25

Stronger IMFs result in…

Answer 25

Higher Boiling and Melting Points

Question 26

Dipole-Dipole

Answer 26

Polar molecules only

Question 27

LDFs

Answer 27

All molecules. Weakest IMF

Question 28

Electrostatic

Answer 28

forces of attraction between charge particles

Question 29

Hydrogen Bonding

Answer 29

H bonded to F, O, N. Strongest IMF

Question 30

Cation

Answer 30

Positively Charged ion

Question 31

Anion

Answer 31

Negatively Charged ion

Question 32

Alloy

Answer 32

A homogenous mixture of metals. Solid Solution. Two types; Substitutional and Interstitial.

Question 33

Substitutional Alloy

Answer 33

The added atoms are similar in size to the original metals atoms and replace some of the original metal atoms.
Brass is a Substitutional Alloy of copper and zinc

Question 34

Interstitial Alloy

Answer 34

The added atoms are smaller than the original metal atoms and fits into the spaces between metal atoms.
Steel is an electrical alloy of Iron and Carbon.

Question 35

Allotrope

Answer 35

A different form of an element in the same physical state with different bonding within the structure.

Question 36

Solubility

Answer 36

Like dissolves Like.
Polar dissolves Polar.
Non polar dissolves Non polar.
Non Polar and Polar do not mix.

Question 37

Conductivity of covalent compounds

Answer 37

Covalent bonds do not conduct due to no mobile ions and electrons are fixed.