Chapter 5 Electrons And Bonding

Question 1

Principle quantum n

Answer 1

The number of shells or energy level

number of electrons= 2n^2

Question 2

Atomic orbitals

Answer 2

A region around the nucleus that can hold up to two electrons, with opposite spins.
s p d and f orbitals which each have a different shape

Question 3

S- orbital

Answer 3

• shape of a sphere
• each she’ll From n=1 contains one s orbital
• the greater the shell number, the greater the radius of its s orbital

Question 4

P- orbital

Answer 4

• shape of a dumb-bell
• 3 separate p- orbitals at right angles to one another
• each shell from n=2 contains 3 p- orbitals
• the greater the shell number the further the p- orbital is from the nucleus

Question 5

D-orbital and f-orbital

Answer 5

• Each shell from n=3 contains 5 d-orbitals

- each shell from n=4 contains 7 f orbitals

Question 6

Sub shells

Answer 6

A group of orbitals of the same type within a shell.

Question 7

Shell

Answer 7

A group of atomic orbitals with the same principal quantum number, n. Also known as a main energy level.

Question 8

electron configuration

Answer 8

A shorthand representation that shows how electrons occupy sub-shells in an atom.

Question 9

cation

Answer 9

A positively charged ion with fewer electrons than protons. formed when atoms lose electrons

Question 10

anion

Answer 10

A negatively charged ion with more electrons than protons. formed when atoms gain electrons

Question 11

ionic bonding

Answer 11

The electrostatic attraction between positive and negative ions.

Question 12

giant ionic lattice

Answer 12

A three-dimensional structure of oppositely charged ions, bonded together by strong ionic bonds.

Question 13

covalent bond

Answer 13

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

Question 14

molecule

Answer 14

The smallest part of a covalent compound that can exist while retaining its chemical
identity, consisting of two or more atoms covalently bonded together.

Question 15

Lone pair

Answer 15

An outer shell pair of electrons that is not involved in chemical bonding.

Question 16

displayed formula

Answer 16

A formula showing the relative positioning of all the atoms in a molecule and the bonds between them.

Question 17

dative covalent/coordinate bond

Answer 17

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only; also called a coordinate bond.

Question 18

Common cations

Answer 18

Na^+, Ca^2+, Al^3+, NH4^+

Question 19

Common anions

Answer 19

Cl^-, O^2-, NO3^- , SO4^2-

Question 20

polar (molecule)

Answer 20

With δ+ and δ– charges at different ends of the molecule.
A molecule with an overall dipole, having taken into account any dipoles across
bonds and the shape of the molecule.

Question 21

Expansion of the octet

Answer 21

When more than 8 electrons in the outer shell in covalent bonding.
This is possible from the n=3 shell (18 electrons can fit in this shell), when a d sub- shell becomes available for the expansion

Question 22

Double bond

Answer 22

The strong electrostatic attraction between two shared pair of electrons and the nuclei of the bonded atoms.