Chapter 2 - Elements and the Periodic Table

Question 1

Alkali Metals

Answer 1

Group 1 on the Periodic Table (Block S). Properties include: highly reactive, malleable, ductile, good conductors, softer than most metals. Reactivity increases as period number increases; form cations with a 1+ charge.

Question 2

Alkaline Earths

Answer 2

Group 2 on the Periodic Table (Block S). Properties include: highly reactive, malleable, ductile, good conductors. Reactivity increases as period number increases; form cations with a 2+ charge.

Question 3

Anion

Answer 3

A negative ion (has more electrons than protons).

Question 4

Cation

Answer 4

A positive ion (has more protons than electrons).

Question 5

Transition Metals

Answer 5

Groups 3-12 on the Periodic Table (Block D). Can put more than 8 electrons in their second most outer shell due to the Aufbau Principle. Colourful!

Question 6

Halogens

Answer 6

Group 17 on the Periodic Table (Block P). Properties include: highly reactive, not found naturally (instead as salts). Reactivity decreases as period number increases; form anions with a 1- charge.

Question 7

Noble Gases

Answer 7

Group 18 on the Periodic Table (Block S for hydrogen; Block P for all others). Properties include: colourless, full outer shells, found naturally in the atmosphere, very stable, don’t react. Density increases as row number increases; don’t form ions.

Question 8

Atom

Answer 8

The fundamental building block of all matter.

Question 9

Atomic Number

Answer 9

The number of protons in the nucleus of an atom; determines the type of atom.

Question 10

Atomic Symbol

Answer 10

One or two letters used to represent a particular element.

Question 11

Atomic Mass

Answer 11

The sum of an atom’s protons and neutrons.

Question 12

Valence Electrons

Answer 12

Electrons that are in an atom’s outer shell.

Question 13

Electron

Answer 13

A subatomic particle with a negative charge; found in orbitals around the nucleus.

Question 14

Electron Configuration

Answer 14

The distribution of electrons within an atom’s subshells and orbitals.

Question 15

Element

Answer 15

A substance made of only one type of atom.

Question 16

Group

Answer 16

A column on the Periodic Table, which determines the number of electrons in an atom’s outer shell.

Question 17

Ion

Answer 17

An atom that has lost or gained electrons, giving it a positive or negative charge.

Question 18

Neutron

Answer 18

A subatomic particle with no charge; found in the nucleus of atoms.

Question 19

Nucleus

Answer 19

The centre of an atom, containing protons and neutrons.

Question 20

Period

Answer 20

A row on the Periodic Table, which determines the number of electron shells an atom has.

Question 21

Periodic Table

Answer 21

A table created by Dmitri Mendeleev that displays elements, their atomic symbol, mass, number, and groups similar elements together.

Question 22

Proton

Answer 22

A subatomic particle with a positive charge; found in the nucleus of atoms.

Question 23

Subatomic Particles

Answer 23

Structures that make up atoms; either protons, neutrons or electrons.

Question 24

Isotopes

Answer 24

An atom that has a different number of protons to neutrons.

Question 25

Reactivity/Valency

Answer 25

The measure of how readily/easily a substance undergoes a chemical reaction.

Question 26

Electronegativity

Answer 26

The measure of how firmly an atom is able to hold onto its valence electrons.

Question 27

Electrostatic Attraction

Answer 27

The bonds between charged particles, such as a positive cation and negative anion.

Question 28

Balmer Series

Answer 28

The visible light energy emitted from a hydrogen atom when electrons fall to n = 2.

Question 29

Paschen Series

Answer 29

The infrared radiation emitted by a hydrogen atom when electrons fall to n = 3.

Question 30

Lyman Series

Answer 30

The ultraviolet radiation emitted by a hydrogen atom when electrons fall to n = 1 (the ground state).

Question 31

Uncertainty Principle

Answer 31

A theory proposed by Werner Heisenberg, which states that the location of an electron cannot be known, only the probability of it being there.

Question 32

Wave-Particle Duality

Answer 32

When a quantum - such as an electron or light - can exist as both a wave and a particle. (Note: quantum = specific amount of something).

Question 33

Orbital

Answer 33

The region of space around an atom where an electron is most likely to exist. Can contain a maximum of 2 electrons.

Question 34

Shell

Answer 34

The main energy levels in an atom.

Question 35

Sub-Shell

Answer 35

Smaller energy levels within the main energy levels of an atom. s, p, d & f.

Question 36

Aufbau Principle

Answer 36

A rule which states that electrons fill lower energy subshells before higher energy subshells.

Question 37

Compound

Answer 37

A substance that contains more than one type of atom.

Question 38

Nucleons

Answer 38

Protons and neutrons referred to collectively.

Question 39

Bohr Model

Answer 39

An atomic theory created by Niels Bohr, which states that:
* Electrons move in fixed orbits called ‘shells’.
* Each shell corresponds to a specific energy level.
* Electrons cannot exist between energy levels.
* Electrons can move between energy levels.
* Orbits of larger radii have higher energy.

Question 40

Ground State

Answer 40

The lowest energy level of an atom (n = 1).

Question 41

Schrodinger Model

Answer 41

An atomic theory created by Erwin Schrondiger, which states that:
* electrons behave like waves
* elections are elusive
* orbitals are the regions of space were electrons could be found
* there are subshells within each shell

Question 42

First Ionisation Energy

Answer 42

The measure of how much energy is required to remove the first electron in an atom.

Question 43

Block (Periodic Table)

Answer 43

One of the four main areas on the periodic table, which have their valence electrons in the same subshell.