Ionic bonds

Open Ended

How do ionic bonds form and how are the ions arranged in an ionic compound?

Multiple Choice

Sodium has 1 valence electron. How many more electrons does it need to fulfill the octet rule?

• 1

• 3

• 5

• 7

Reorder

Reorder the following from LEAST to MOST valence electrons

• hydrogen

• magnesium

• aluminum

• carbon

• sulfur

1

2

3

4

5

• 1
• 2
• 3
• 4
• 5

Multiple Choice

Is this correct way to draw the Lewis Dot Structure for Carbon?

• Yes

• No, too many electrons

• No, not enough electrons

• No, dots are in wrong places

Open Ended

The Lewis dot structure for oxygen (O) has _______ valence electrons.

Open Ended

How many more electrons does Hydrogen need to have a full valence shell?

Fill in the Blanks

How many electrons complete the valence shell for a Hydrogen atom

Fill in the Blanks

This is a Bohr Diagram of Aluminum. How many total electrons does Aluminum have?

Multiple Choice

N-3 is formed. What is the correct equation for this ion formation?

• $$N^{+3}\ \longrightarrow N^{-3}\ +\ 3\ e$$

• $$N\ +3e\ \longrightarrow N^{-3}$$

• $$N\ +\ 2\ e\ \longrightarrow N^{-2}\$$

• $$N^{+3}\ \ +\ 3\ e\longrightarrow N^{-3}\$$

Multiple Choice

The chemical reactivity of metals is primarily due to their:

• High melting points

• Ability to lose valence electrons easily

• Ability to gain electrons easily

• Low density

Multiple Choice

The general electronic configuration [Rn]5f^1-14 6d^0-1 7s² is of -:

• Lanthanoids

• Actinoids

• s- block elements

• d-block elements

Multiple Choice

Transition metal have variable oxidation states due to

• ability to lose electron from 3d and 4s
• ability to lose electrons from 4s
• ability to form complex ions
• ability to react with ligands

Categorize

Options (6)

N⁺⁵ has 2 electrons

N⁺⁵ has 10 electrons

Same electron configuration as He in the ground state

Same electron configuration as Ne in the ground state

It is an ion

It is an atom

Categorize as true or false about N⁺⁵?

True

False

Fill in the Blanks

Na⁺¹ (a sodium ion) has a total of

electrons.

Multiple Choice

What are the stable electron arrangements referred to as in transition metal ions?

• noble gas configurations

• pseudo-noble gas configurations

• octet configurations

• stable gas configurations

Multiple Choice

Which group of elements tends to gain 3 electrons to form an anion with a 3- charge?

• Group 15

• Group 16

• Group 17

• Group 14

Multiple Choice

Name this ionic compound: Al₂O₃

• Dialuminum oxide

• Aluminum oxygen

• Oxygen Aluminide

• Aluminum oxide

Multiple Choice

Which of these is the correct match to form an ionic compound?

Multiple Select

Select all the true statements:

• Each outer shell electron in Cl is represented by a cross.

• In Na, the total charge is -2.

• Na+ and Cl- are held together by electrostatic attraction.

• Na+ has a full outer shell of electrons.

Fill in the Blanks

Key Ideas: Ionic compounds are made from negative ions(_____) attracting to positive ions(_____) forming a (_____) structure.

Multiple Choice

Why do ionic compounds have high melting and boiling points?

• Their ions are free to move.

• Their ions are held in fixed positions.

• They have many strong bonds which require a large amount of heat energy to overcome these strong bonds.

• They have weak bonds which require a little amount of heat energy to overcome these weak bonds.

Multiple Choice

This is an image of the giant ionic lattice representing Sodium Chloride, what is represented by the positive sign (+)?

• Cl cation

• Cl anion

• Na cation

• Na anion

Multiple Choice

The three dimensional arrangement of a solid crystal.

• Crystal

• Crystal System

• Crystal Lattice

• Cube

Multiple Choice

What is the relationship between ionic radius and lattice energy as illustrated in the image?

• Smaller ionic radius leads to greater lattice energy

• Larger ionic radius leads to greater lattice energy

• Ionic radius has no effect on lattice energy

• Lattice energy is only affected by charge

Poll

How confident do you feel about this topic now?

• Very confident
• Somewhat confident
• Not confident