Lecture 3 -the Periodic Table

Question 1

What is the aim of Topic 3 – The Periodic Table?

Answer 1

Revise nomenclature and chemical calculations, understand trends and groups of elements, determine electron configurations, and calculate electrons in ions.

Question 2

Elements in the periodic table are arranged in order of increasing _______.

Answer 2

[atomic number]

Question 3

What are the vertical columns in the periodic table called?

Answer 3

[groups]

Question 4

What are the horizontal rows in the periodic table called?

Answer 4

[periods]

Question 5

Elements in the same group have _______ chemical properties.

Answer 5

[similar]

Question 6

What is the atomic radius?

Answer 6

The total distance from the nucleus of an atom to the outermost orbital of its electron.

Question 7

What is the trend of atomic radius within a group on the periodic table?

Answer 7

Atomic radius increases from top to bottom.

Question 8

What causes the atomic radius to increase when moving down a group?

Answer 8

The increase in the principal energy number (n) of the outer electrons.

Question 9

What is the trend of atomic radius within a period on the periodic table?

Answer 9

Atomic radius decreases from left to right.

Question 10

What is effective nuclear charge (Z_eff)?

Answer 10

The net positive charge attracting an electron in an atom.

Question 11

How is effective nuclear charge approximated?

Answer 11

Z_eff = Z - S, where Z is the atomic number and S is the number of shielding electrons.

Question 12

What is electronegativity?

Answer 12

The measure of the ability of an atom in a chemical compound to attract electrons from another compound.

Question 13

Which element is the most electronegative?

Answer 13

Fluorine (F) with a value of 4.0.

Question 14

What is the trend in electronegativity within a period?

Answer 14

Electronegativity increases from left to right.

Question 15

What is the trend in electronegativity down a group?

Answer 15

Electronegativity decreases from top to bottom.

Question 16

What is bond polarity?

Answer 16

The concept that describes the sharing of electrons between atoms.

Question 17

In a non-polar covalent bond, how are electrons shared?

Answer 17

Electrons are shared equally between two atoms.

Question 18

What is the octet rule?

Answer 18

Stability comes from having a full outer shell of electrons, typically eight.

Question 19

What are alkali metals?

Answer 19

Group 1 elements that have one electron in the outermost shell.

Question 20

What is the electron configuration of Lithium (Li)?

Answer 20

1s² 2s¹

Question 21

What happens to the atomic radius when forming cations?

Answer 21

The radius decreases because there is one less shell of electrons.

Question 22

Which group of elements is known as alkaline earth metals?

Answer 22

[Group 2]

Question 23

What is the general trend for ionic radii in groups?

Answer 23

Atomic and ionic radii increase as you go down the group.

Question 24

What are transition metals known for?

Answer 24

High melting points and the ability to exist in a range of oxidation states.

Question 25

What is the electron configuration notation for Magnesium (Mg)?

Answer 25

[Ne] 3s²

Question 26

What principle states that electrons will occupy the lowest energy orbitals first?

Answer 26

[Aufbau principle]

Question 27

What is Hund's rule?

Answer 27

No two electrons with the same spin can occupy the same orbital.

Question 28

What is the maximum number of electrons per orbital?

Answer 28

Two electrons.

Question 29

What does the Pauli exclusion principle state?

Answer 29

No two electrons in an atom can have the same set of quantum numbers.

Question 30

What is the electron configuration of Neon (Ne)?

Answer 30

1s² 2s² 2p⁶

Question 31

Which group forms M³⁺ ions?

Answer 31

[Group 13 (III)]

Question 32

What are the elements in Group 15 known as?

Answer 32

[Pnictogens]

Question 33

What type of bond forms when the difference in electronegativity is large enough?

Answer 33

[Ionic bond]

Question 34

What is the electron configuration of Arsenic (As)?

Answer 34

[Ar] 4s² 3d¹⁰ 4p³

Question 35

What is the primary characteristic of metalloids?

Answer 35

Having properties intermediate between metals and non-metals.

Question 36

What is the electron configuration for Neon?

Answer 36

1s² 2s² 2p⁶

Question 37

What is the electron configuration for Fluorine?

Answer 37

1s² 2s² 2p⁵

Question 38

What is the electron configuration for Beryllium?

Answer 38

1s² 2s²

Question 39

What is the electron configuration for Sodium?

Answer 39

1s² 2s² 2p⁶ 3s¹

Question 40

What is the electron configuration for Zinc?

Answer 40

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s²

Question 41

What is ionisation energy?

Answer 41

Minimum energy required to remove an electron from the ground state of an isolated gaseous atom or ion.

Question 42

What is the first ionisation energy (I₁)?

Answer 42

Energy required to remove one electron from a gaseous neutral atom.

Question 43

What is the second ionisation energy (I₂)?

Answer 43

Energy required to remove a second electron from a cation.

Question 44

True or False: The greater the ionisation energy, the easier it is to remove an electron.

Answer 44

False

Question 45

What are positive ions called?

Answer 45

Cations

Question 46

What are negative ions called?

Answer 46

Anions

Question 47

What is the symbol for Sodium in its neutral state?

Answer 47

Na

Question 48

What is the ion form of Magnesium?

Answer 48

Mg²⁺

Question 49

What is the ion form of Oxygen?

Answer 49

O²⁻

Question 50

Fill in the blank: Ions can gain or lose up to ______ electrons.

Answer 50

3

Question 51

Which group of elements loses one electron to become +1 ions?

Answer 51

Group One

Question 52

Which group of elements loses two electrons to become +2 ions?

Answer 52

Group Two

Question 53

What type of ions do Transition Metals typically form?

Answer 53

+1, +2, or +3

Question 54

What do Group Five (15) elements do to become ions?

Answer 54

Gain three electrons

Question 55

What do Group Six (16) elements do to become ions?

Answer 55

Gain two electrons

Question 56

What do Group Seven (17) elements do to become ions?

Answer 56

Gain one electron

Question 57

What do Noble Gases (Group Eight) do in terms of ion formation?

Answer 57

Do not gain or lose electrons

Question 58

Calculate the electron loss/gain of Lithium: ______

Answer 58

+1

Question 59

Calculate the electron loss/gain of Nitrogen: ______

Answer 59

-3

Question 60

Calculate the electron loss/gain of Argon: ______

Answer 60

0

Question 61

Calculate the electron loss/gain of Magnesium: ______

Answer 61

+2

Question 62

Calculate the electron loss/gain of Gallium: ______

Answer 62

+3

Question 63

Give an example of an ionic compound formed between Group One and the halogens.

Answer 63

NaCl (Sodium Chloride)

Question 64

Give an example of an ionic compound formed between Group Two and a Group 16 element.

Answer 64

CaO (Calcium Oxide)

Question 65

Give an example of an ionic compound formed between the transition metal ion Fe³⁺ and a Group 17 element.

Answer 65

FeCl₃ (Iron(III) Chloride)