Chapter 1- Atomic structure and chemical bonding

Question 1

A subatomic particle, symbol p or p+, with a positive electric charge of +1 elementary charge and a mass slightly less than that of a neutron.

Answer 1

Proton

Question 2

A subatomic particle, symbol n or n0, with no net electric charge and a mass slightly larger than that of a proton.

Answer 2

Neutron

Question 3

It plays as an essential role in numerous physical phenomena, such as electricity, magnetism, chemistry and thermal conductivity, and they also participate in gravitational, electromagnetic and weak interactions.

Answer 3

Electron

Question 4

It represents the number of protons in the nucleus of an atom.

Answer 4

Atomic number

Question 5

The total number of protons and neutrons in the nucleus of an atom.

Answer 5

Mass number

Question 6

Atoms of the same element having the same atomic number but different atomic masses.

Answer 6

Isotopes

Question 7

Atoms of different elements having the same mass number but different atomic numbers.

Answer 7

Isobars

Question 8

Atoms of different elements having the same number of neutrons but differ in atomic numbers and mass numbers.

Answer 8

Isotones

Question 9

It is the space around the nucleus in which the electron is found with a probability of 90%.

Answer 9

Orbital

Question 10

The number of electrons in an atom are arranged in shells or ‘energy levels’ around the nucleus

Answer 10

Shells

Question 11

Electrons are those seen in the previous noble gas and any completed transition series. They fill all the lower energy levels of an atom.

Answer 11

Inner (core) electrons

Question 12

Are those in the highest energy level (highest n value). They spend most of their time farthest from the nucleus.

Answer 12

Outer electrons

Question 13

Involved in forming compounds. Among the main group elements, the valence electrons are the outer electrons.

Answer 13

Valence electrons

Question 14

It is a region of space within an electron shell that contains electrons that have the same energy.

Answer 14

Subshell

Question 15

Describes the size of orbitals and relative distance of the electrons from the nucleus.

Answer 15

Principal quantum number

Question 16

This refers to the shape of the orbitals.

Answer 16

Angular momentum quantum number

Question 17

Refers to the orientation of the orbitals in space around the nucleus.

Answer 17

Magnetic quantum number

Question 18

Describes the spin of electrons in an orbital which is opposite direction to differentiate one electron from the other in the same orbital.

Answer 18

Spin quantum number

Question 19

The distribution of electrons in the energy levels and sublevels of an atom

Answer 19

Electron configuration

Question 20

The number of different states of equal energy.

Answer 20

Degree of degeneracy or degeneracy

Question 21

Electron orbitals that have the same energy levels.

Answer 21

Degenerate orbitals

Question 22

A property of a substance to be slightly attracted to a magnetic field. It is exhibited by substances that contain one or more unpaired electrons.

Answer 22

Paramagnetism

Question 23

A property of a substance to be slightly repelled by a magnetic field. It is exhibited by substances whose electrons are all paired.

Answer 23

Diamagnetism

Question 24

Electrons first occupy the lowest energy orbitals available to them; only when the lower-energy orbitals are filled that they enter higher–energy orbitals.

Answer 24

Aufbau (building–up) principle

Question 25

Only two electrons having opposite spins can occupy an orbital. The third electron will eventually be repelled.

Answer 25

Pauli’s exclusion principle

Question 26

Electrons distribute singly before pairing.

Answer 26

Hund’s rule

Question 27

These gases have complete e- configuration of ns2np6 except for He making them difficult to either gain or loss electrons.

Answer 27

Electron configuration of noble gases

Question 28

The arrangement of electrons around the nucleus of an atom with lower energy levels.

Answer 28

The ground state

Question 29

Any state other than the ground state of an atom or molecule; a state that has higher energy than the ground state.

Answer 29

Excited state-

Question 30

An elevation in energy level above an arbitrary baseline energy state.

Answer 30

Excitation

Question 31

The electrostatic force which holds the atoms in a compound or molecule. This results from the gain and loss of electrons, or from the sharing of electrons between atoms.

Answer 31

Chemical bond-

Question 32

The ability of an atom to form bonds.

Answer 32

Valance.

Question 33

States that atoms are most stable when they have a full shell of electrons in the outside electron shell.

Answer 33

Octet rule

Question 34

It is a chemical bond resulting from the mutual attraction of oppositely charged ions.

Answer 34

Ionic bonding

Question 35

Formed from the force of electrostatic attraction between oppositely charged ions (cations and anions).

Answer 35

Ionic bonding

Question 36

It is an electrically charged atom of an element or group of atoms that carries an electrical charge.

Answer 36

Ion

Question 37

It is a positively charged atom of an element. It is formed when an atom loses electron (s).

Answer 37

Cation

Question 38

A negatively charged atom of an element. It is produced when an atom gains electron(s).

Answer 38

Anion

Question 39

Formed when atoms share a pair of electrons to form covalent molecules.

Answer 39

Covalent

Question 40

Bond formed when the combining atoms have a big difference in their electronegativity values, and that the sharing of the electrons is not equal.

Answer 40

Polar covelant bond

Question 41

This type of bond is formed from the combination of atoms of the same element or atoms whose electronegativity values are very close.

Answer 41

Non-polar covalent bond

Question 42

A type of covalent bond where the two electrons in the bond are only donated by a single atom.

Answer 42

Coordinate covalent bond

Question 43

Shows the valence electrons in an element.

Answer 43

Lewis structure

Question 44

States that the bond energy is inversely related to the bond length (r), and so factors which influence a bond's strength influence its length.

Answer 44

Coulomb's law

Question 45

The number of electrons that an atom will lose or gain in order to get stable electronic configuration in forming ionic bond.

Answer 45

Electrovalency

Question 46

The number of electrons that an atom can share to get a stable electronic configuration.

Answer 46

Covalency:

Question 47

The energy required to remove an electron from a neutral atom.

Answer 47

Ionization potential

Question 48

The energy released when an atom gains one electron to the element.

Answer 48

Electron affinity

Question 49

A measure of the ability of an atom in a molecule to attract electrons to itself.

Answer 49

Electronegativity