The Periodic Table, Atoms and Ions

Question 1

How are elements ordered in the periodic table?

Answer 1

Elements are listed in order of increasing atomic number

Question 2

Where are elements with similar properties placed in a periodic table?

Answer 2

Elements with similar properties are placed in the same column(Group)

Question 3

What is the Atomic Number?

Answer 3

The Atomic Number is the number of protons in the nucleus

Question 4

What is the Atomic Mass?

Answer 4

The Atomic Mass is the number of protons and neutrons in the nucleus

Question 5

What does a Chemical element consist of?

Answer 5

A chemical element consists of atoms with the same number of protons

Question 6

What is an isotope?

Answer 6

Isotopes are forms of an element that have the same atomic number but different number of neutrons

Question 7

How many elements are required for a human to conduct a healthy life?

Answer 7

Humans need 25 elements to conduct a healthy life

Question 8

What is periodicity?

Answer 8

Periodicity is the name given to the gradual change of physical and chemical properties in elements in the same group

Question 9

What is an element?

Answer 9

An element is a single substance that cannot be split into any separate substances by chemical means

Question 10

What is the smallest unit an element can exist in?

Answer 10

The smallest unit an element can exist in is an atom

Question 11

What is an atom?

Answer 11

An atom is defined as the smallest particle into which an element can be divided

Question 12

What are the subatomic particles?

Answer 12

The subatomic particles are; Protons, Neutrons and Electrons

Question 13

What charge does a proton carry?

Answer 13

A proton carries a single positive charge

Question 14

What charge does an electron carry?

Answer 14

An electron carries a single negative charge

Question 15

What charge does a neutron carry?

Answer 15

A neutron carries no charge

Question 16

What happens if the number of electrons is different from the number of protons?

Answer 16

If the number of electrons is different to the number of protons, a charged ion is formed

Question 17

What happens if an ion gains one or more electrons?

Answer 17

If an atom gains one or more electrons, it becomes a negative ion, known as an Anion

Question 18

What happens if an atom loses one or more electrons?

Answer 18

If an atom loses one or more electrons, it becomes a positive ion, known as a Cation

Question 19

What does an elements ionization energy tell us?

Answer 19

An elements ionisation energy tells us how readily the element will lose an electron to become a positively charged ion

Question 20

Elements on the left of the periodic table have what type of ionization energy?

Answer 20

Elements on the left side of the periodic table have relatively low ionization energies, and readily form positively charged ions

Question 21

Elements on the right of the periodic table have what type of ionization energy?

Answer 21

Elements on the right side of the periodic table have relatively high ionization energies, and are very unlikely to form positively charged ions. Instead, they readily form negatively charged ions by accepting an electron

Question 22

What is the difference between isotopes of the same element?

Answer 22

Different isotopes of the same element have different mass numbers but retain the same atomic number

Question 23

What is an elements relative atomic mass?

Answer 23

An elements relative atomic mass is a measure of the average mass of an atom of that element

Question 24

What types of atomic orbital are there?

Answer 24

There are 4 different types of atomic orbitals:
S orbitals
P orbitals
D orbitals
F orbitals

Question 25

What are orbitals grouped into?

Answer 25

Orbitals are grouped into shells

Question 26

What are equivalent orbitals occupying the same shell grouped into?

Answer 26

Equivalent orbitals occupying the same shell are grouped into subshells

Question 27

What happens when the electrons in the atom are further away form the nucleus?

Answer 27

Electrons have progressively higher energy as the distance from the nucleus of the shell they occupy increases

Question 28

What orbitals are filled first? Low energy or High Energy?

Answer 28

Low energy orbitals become filled with electrons before high-energy orbitals

Question 29

What are degenerate orbitals?

Answer 29

Degenerate orbitals are orbitals that have the same energy levels

Question 30

How are degenerate orbitals filled?

Answer 30

Each degenerate orbital in a subshell must be occupied by one electron before any one of the orbitals becomes completely filled

Question 31

What is the valence shell?

Answer 31

The valence shell is the shell furthest from the nucleus

Question 32

What are electrons contained in the valence shell called?

Answer 32

Electrons held in the valence shell are known as valence electrons

Question 33

What do the elements from the same group have in common?

Answer 33

Elements from the same group in the periodic table have the same number of Valence Electrons

Question 34

What can happen when an atom absorbs energy?

Answer 34

When an atom absorbs energy, electrons can jump between orbitals of different energy

Question 35

What is the energy of electromagnetic radiation determined by?

Answer 35

The energy of electromagnetic radiation is determined by its wavelength

Question 36

What wavelength does high-energy radiation have?

Answer 36

High-energy radiation has a short wavelength

Question 37

What wavelength does low-energy radiation have?

Answer 37

Low-energy radiation has a long wavelength

Question 38

What is the bond length?

Answer 38

The bond length is the sum of the atomic radii of two covalently bonded atoms

Question 39

What is the atomic radius

Answer 39

The atomic radius is half the distance between the nuclei of two identical atoms, when joined by a single covalent bond

Question 40

What does VSEPR Theory stand for?

Answer 40

Valence Shell Electron Pair Repulsion

Question 41

How do you use the VSEPR Theory?

Answer 41

To use VSEPR theory, we count the number of pairs of bonding electrons plus the number of non-bonding pairs around the central atom

Question 42

What type of bond does a single bond contain?

Answer 42

A single bond contains 1 sigma bond

Question 43

What type of bonds does a double bond contain?

Answer 43

A double bond contains 1 sigma bond and 1 pi bond

Question 44

What type of bonds does a triple bond contain?

Answer 44

A triple bond contains 1 sigma bond and 2 pi bonds

Question 45

What do we need to consider when using VSEPR theory to predict molecular shape in compounds containing double and triple bonds?

Answer 45

We only need to consider the number of valence electrons occupying single bonds

Question 46

What does the arrangement of Valence Electrons predicted by VSEPR theory occur from a result of?

Answer 46

The arrangement of Valence Electrons predicted by VSEPR theory occurs as a result of the hybridization of atomic orbitals to form hybrid orbitals

Question 47

What undergoes overlap to form single covalent bonds?

Answer 47

It is the Hybrid Orbitals that undergo overlap to form single covalent bonds

Question 48

The number of hybrid orbitals formed after hybridization is equal to what?

Answer 48

The number of atomic orbitals undergoing hybridization

Question 49

What happens when one s and three p orbitals undergo sp^3 hybridization?

Answer 49

They form four sp^3 hybrid orbitals with tetrahedral geometry; They can participate in 4 sigma bonds

Question 50

What happens when one s and two p orbitals undergo sp^3 hybridization?

Answer 50

They form three sp^3 hybrid orbitals with typical planar geometry; They can participate in 3 sigma bonds

Question 51

What happens when one s and one p orbitals undergo sp^3 hybridization?

Answer 51

They form two sp^3 orbitals with linear geometry; They can participate in 2 sigma bonds

Question 52

What undergoes overlap to form pi bonds?

Answer 52

Unhybridized orbitals overlap to form pi bonds

Question 53

What can be treated as being equivalent when atomic orbitals hybridize

Answer 53

Non-bonding pairs of valence electrons and bonding pairs of valence electrons(sigma bonds) can be treated as being equivalent

Question 54

What does a molecules configuration describe?

Answer 54

A molecules configuration describes how its composite atoms are joined together, and is fixed

Question 55

What does a molecules conformation describe?

Answer 55

A molecules conformation describes how its composite atoms are arranged at particular moments in time, and is variable

Question 56

Where is rotation not possible?

Answer 56

Rotation is not possible about double or triple bonds, or where delocalization occurs

Question 57

What is steric hindrance?

Answer 57

Steric Hindrance is the restriction of movement due to a lack of space between neighbouring atoms

Question 58

What shape are Porphyrins?

Answer 58

Porphyrins are ring-shaped

Question 59

What can pigments derived from porphyrins be called?

Answer 59

Porphyrin-derived pigments can be called the "colours of life". In the sense that these rings are necessary to sustain key activities in nearly all organisms

Question 60

What enzyme is the last enzyme before a major breaking point in the synthesis of the "rings of life"

Answer 60

Protoporphyrin oxidase

Question 61

Where is protoporphyrin oxidase bound to in Animal cells?

Answer 61

In Animal cells, protoporphyrin oxidase is bound to the inner membrane of mitochondria

Question 62

What do non-bonding pairs do to a greater extent that bonding pairs?

Answer 62

Non-bonding pairs repel neighbouring valence electrons to a greater extent than bonding pairs, making bond angles smaller than we would otherwise expect for a given geometry