4.1 - Ions

Last updated over 4 years ago

24 questions

1

Library

4.1 - Ions

Last updated over 4 years ago

24 questions

Ions
Objectives: 
Describe how valence electrons are involved in ionic bonding.
Calculate the number of protons, neutrons, electrons, mass number and charge of an ion.
Predict the type of ion that an atom will form based on the atom’s location on the periodic table.
Predict how ions are "held" together in order to form an ionic bond. 

WHY?

When electrons are transferred between two atoms, those atoms are now considered an ion. Many atoms present in nature are not in their 'atom' form, but in their 'ion' form.  The ion an atom forms is dependent on its number of valence electrons, and force of attraction between the nucleus and the electrons.  In this part of the activity, you will determine what an ion is and how they are formed.

DIRECTIONS: Use the "Atom" screen on the simulation to answer questions 1-8. 

If you'd like to have 'Build an Atom' open in a different window, click on the following link: Build an Atom

1

Using what you learned from the simulation, define the term 'ion' in your own words.

1

Think about your answer to the previous question. Why do you think lithium always forms a +1 ion, beryllium always forms a +2 ion, and boron always forms a +3 ion?

1

Think about your to the previous question. Why do you think fluorine always forms a -1 ion, oxygen always forms a -2 ion, and nitrogen always forms a -3 ion?

Optional: Did you struggle answering the past questions? Especially questions 5 & 8? Check out this video! 

1

Using a Periodic Table, fill in the table in the "Show Your Work" box to demonstate how the ions listed form.

If you are not sure how to fill in the chart, check out this video!

Note: You do not need to draw the protons, you can just write the number of protons in the nucleus!

1

CHECK THIS OUT BEFORE MOVING ON! 

What is referred to as a "Group" on the Periodic Table:  

What is referred to as a "Period" on the Periodic Table: 

1

Using a Periodic Table, complete the table in the "Show Your Work" box to summarize the patterns between the ions that form and the location of elements on the periodic table. The first row is done for you.

HINT: For the 'Will atom gain or lose electrons?' column, consider the number of electrons the atom has and the number of electrons that would need to be lost or gained in order to create an ion. For example, it is far easier for a lithium atom to lose one electron than it is to gain seven.

If you are not sure how to fill in the chart, check out this video!

Consider your answers to #11 as you answer questions 12-17.

1

If you are unsure of your previous answers, check out this video! 

1

Draggable item		Corresponding Item

1

The animation below shows the steps involved in forming an ionic bond. (We'll be learning about these next!!)

Analyze the animation below. How are ions that form ionic bonds held together?

1

Explain why an ionic bond typically forms between a metal and a nonmetal.

Ions
Objectives: 
Describe how valence electrons are involved in ionic bonding.
Calculate the number of protons, neutrons, electrons, mass number and charge of an ion.
Predict the type of ion that an atom will form based on the atom’s location on the periodic table.
Predict how ions are "held" together in order to form an ionic bond. 

WHY?

When electrons are transferred between two atoms, those atoms are now considered an ion. Many atoms present in nature are not in their 'atom' form, but in their 'ion' form.  The ion an atom forms is dependent on its number of valence electrons, and force of attraction between the nucleus and the electrons.  In this part of the activity, you will determine what an ion is and how they are formed.

DIRECTIONS: Use the "Atom" screen on the simulation to answer questions 1-8. 

If you'd like to have 'Build an Atom' open in a different window, click on the following link: Build an Atom

What is the difference between a neutral atom and an ion?

In an ion, the number of protons is the same as the number of electrons.  In a neutral atom, the number of protons is different from the number of electrons.

In a neutral atom, the number of protons is the same as the number of electrons.  In an ion, the number of protons is different from the number of electrons.

In a neutral atom, the number of neutrons is the same as the number of electrons.  In an ion, the number of neutrons is different from the number of electrons.

In an ion, the number of neutrons is the same as the number of electrons.  In an ion, the number of neutrons is different from the number of electrons.

Using what you learned from the simulation, define the term 'ion' in your own words.

Use the simulation to build a stable, neutral He atom and the following stable ions: Li1+, Be2+, B3+. Draw the atoms or ions in the 'show your work' area, then identify the number of protons and electrons in the atom/ions. You need to click the stable/unstable box in the bottom right corner of the simulation.

(You may simply write the number of protons and neutrons in the nucleus, but please draw the electrons!)

5 electrons
4 protons
3 electrons
3 protons
5 protons
4 electrons
2 protons
2 electrons

Stable atom of helium (He)
Stable ion of lithium (Li1+)
Stable ion of beryllium (Be2+)
Stable ion of boron (B3+)

What do you notice about the number of electrons in Li1+, Be+2, B3+, and He?

There is nothing similar about the ions/atom listed above.

The number of electrons in each ion/atom is equal to the number of protons for that atom/ion.

The number of neutrons in each ion/atom is equal to the number of electrons for that atom/ion.

All of the ions/atom listed above have two electrons.

Think about your answer to the previous question. Why do you think lithium always forms a +1 ion, beryllium always forms a +2 ion, and boron always forms a +3 ion?

Use the simulation to build a stable, neutral Ne atom and the following stable ions: F1-, O2-, N3-. Draw the atoms or ions in the 'show your work' area, then identify the number of protons and electrons in the atom/ions. You need to click the stable/unstable box in the bottom right corner of the simulation.

(You may simply write the number of protons and neutrons in the nucleus, but please draw the electrons!)

7 protons
8 protons
10 protons
7 electrons
10 electrons
8 electrons
9 protons
9 electrons

Stable atom of Ne
Stable atom of F (F1-)
Stable atom of O (O2-)
Stable atom of N (N3-)

What do you notice about the number of electrons in F1-, O2-, N3-, and Ne?

The number of electrons in each ion/atom is equal to the number of protons for that atom/ion.

The number of neutrons in each ion/atom is equal to the number of electrons for that atom/ion.

There is nothing similar about the ions/atom listed above.

All of the ions/atom listed above have ten electrons.

Think about your to the previous question. Why do you think fluorine always forms a -1 ion, oxygen always forms a -2 ion, and nitrogen always forms a -3 ion?

Optional: Did you struggle answering the past questions? Especially questions 5 & 8? Check out this video! 

Using a Periodic Table, fill in the table in the "Show Your Work" box to demonstate how the ions listed form.

If you are not sure how to fill in the chart, check out this video!

Note: You do not need to draw the protons, you can just write the number of protons in the nucleus!

Consider the ions you analyzed in the previous question. How could you calculate the charge of an ion?

THINK! Focus on one of the ions from the previous question and use the formulas below to calculate the charge. The formula that equals the correct charge is the correct formula.

None of these describe how to calculate the charge of an ion.

Charge = (# of protons) + (# of electrons)

Charge = (# of electrons) - (# of protons)

Charge = (# of protons) - (# of electrons)

CHECK THIS OUT BEFORE MOVING ON! 

What is referred to as a "Group" on the Periodic Table:  

What is referred to as a "Period" on the Periodic Table: 

Using a Periodic Table, complete the table in the "Show Your Work" box to summarize the patterns between the ions that form and the location of elements on the periodic table. The first row is done for you.

HINT: For the 'Will atom gain or lose electrons?' column, consider the number of electrons the atom has and the number of electrons that would need to be lost or gained in order to create an ion. For example, it is far easier for a lithium atom to lose one electron than it is to gain seven.

If you are not sure how to fill in the chart, check out this video!

Consider your answers to #11 as you answer questions 12-17.

Elements in groups 1, 2, and 13 often form cations, while elements in groups 15, 16, and 17 often form anions. Considering this, which of the following are the best definitions for cation and anion?

A cation is an ion that has more protons than electrons and is positively charged.  An anion is an ion that has more electrons than protons and is negatively charged.

A cation is an ion that has more protons than electrons and is negatively charged.  An anion is an ion that has more electrons than protons and is positively charged.

A cation is an ion that has more protons than neutrons and is positively charged.  An anion is an ion that has more electrons than neutrons and is negatively charged.

A cation is an ion that has more neutrons than electrons and is positively charged.  An anion is an ion that has more neutrons than electrons and is negatively charged.

Consider what you learned in the last lesson about metals and nonmetals.

Which of the following statements about ions is correct?

Metals tend to lose electrons and form negative ions.  Nonmetals tend to gain electrons and form positive ions.

Metals tend to gain electrons and form positive ions.  Nonmetals tend to lose electrons and form negative ions.

Metals tend to gain electrons and form negative ions.  Nonmetals tend to lose electrons and form positive ions.

Metals tend to lose electrons and form positive ions.  Nonmetals tend to gain electrons and form negative ions.

If you are unsure of your previous answers, check out this video! 

First, complete the table in the 'show your work' box. You must complete EVERY box, not just the colored boxes!

Next, match the colored boxes with the number that you wrote in the box.

Draggable item		Corresponding Item
anion
2+
79
36
80
cation
22
10
19

The animation below shows the steps involved in forming an ionic bond. (We'll be learning about these next!!)

Analyze the animation below. How are ions that form ionic bonds held together?

Explain why an ionic bond typically forms between a metal and a nonmetal.

What is the difference between a neutral atom and an ion?

In an ion, the number of protons is the same as the number of electrons.  In a neutral atom, the number of protons is different from the number of electrons.

In a neutral atom, the number of protons is the same as the number of electrons.  In an ion, the number of protons is different from the number of electrons.

In a neutral atom, the number of neutrons is the same as the number of electrons.  In an ion, the number of neutrons is different from the number of electrons.

In an ion, the number of neutrons is the same as the number of electrons.  In an ion, the number of neutrons is different from the number of electrons.

Use the simulation to build a stable, neutral He atom and the following stable ions: Li1+, Be2+, B3+.  Draw the atoms or ions in the 'show your work' area, then identify the number of protons and electrons in the atom/ions. You need to click the stable/unstable box in the bottom right corner of the simulation. 

(You may simply write the number of protons and neutrons in the nucleus, but please draw the electrons!)

5 electrons

4 protons

3 electrons

3 protons

5 protons

4 electrons

2 protons

2 electrons

Stable atom of helium (He)

Stable ion of lithium (Li1+)

Stable ion of beryllium (Be2+)

Stable ion of boron (B3+)

What do you notice about the number of electrons in Li1+, Be+2, B3+, and He?

There is nothing similar about the ions/atom listed above.

The number of electrons in each ion/atom is equal to the number of protons for that atom/ion.

The number of neutrons in each ion/atom is equal to the number of electrons for that atom/ion.

All of the ions/atom listed above have two electrons.

Use the simulation to build a stable, neutral Ne atom and the following stable ions: F1-, O2-, N3-.  Draw the atoms or ions in the 'show your work' area, then identify the number of protons and electrons in the atom/ions. You need to click the stable/unstable box in the bottom right corner of the simulation.

(You may simply write the number of protons and neutrons in the nucleus, but please draw the electrons!)

7 protons

8 protons

10 protons

7 electrons

10 electrons

8 electrons

9 protons

9 electrons

Stable atom of Ne

Stable atom of F (F1-)

Stable atom of O (O2-)

Stable atom of N (N3-)

What do you notice about the number of electrons in F1-, O2-, N3-, and Ne?

The number of electrons in each ion/atom is equal to the number of protons for that atom/ion.

The number of neutrons in each ion/atom is equal to the number of electrons for that atom/ion.

There is nothing similar about the ions/atom listed above.

All of the ions/atom listed above have ten electrons.

Consider the ions you analyzed in the previous question.  How could you calculate the charge of an ion?

THINK! Focus on one of the ions from the previous question and use the formulas below to calculate the charge. The formula that equals the correct charge is the correct formula.

None of these describe how to calculate the charge of an ion.

Charge = (# of protons) + (# of electrons)

Charge = (# of electrons) - (# of protons)

Charge = (# of protons) - (# of electrons)

What charge do group 1 elements form when they form ions?

What charge do group 2 elements form when they form ions?

What charge do group 13 elements form when they form ions?

What charge do group 15 elements form when they form ions?

What charge do group 16 elements form when they form ions?

What charge do group 17 elements form when they form ions?

Notice that you were not asked to determine the charges of ions formed with elements in Group 14. Why do you think this is?

Notice that you were not asked to determine the charges of ions formed with elements in Group 18. Why do you think this is?

Elements in groups 1, 2, and 13 often form cations, while elements in groups 15, 16, and 17 often form anions.  Considering this, which of the following are the best definitions for cation and anion?

A cation is an ion that has more protons than electrons and is positively charged.  An anion is an ion that has more electrons than protons and is negatively charged.

A cation is an ion that has more protons than electrons and is negatively charged.  An anion is an ion that has more electrons than protons and is positively charged.

A cation is an ion that has more protons than neutrons and is positively charged.  An anion is an ion that has more electrons than neutrons and is negatively charged.

A cation is an ion that has more neutrons than electrons and is positively charged.  An anion is an ion that has more neutrons than electrons and is negatively charged.

Consider what you learned in the last lesson about metals and nonmetals.

Which of the following statements about ions is correct?

Metals tend to lose electrons and form negative ions.  Nonmetals tend to gain electrons and form positive ions.

Metals tend to gain electrons and form positive ions.  Nonmetals tend to lose electrons and form negative ions.

Metals tend to gain electrons and form negative ions.  Nonmetals tend to lose electrons and form positive ions.

Metals tend to lose electrons and form positive ions.  Nonmetals tend to gain electrons and form negative ions.

First, complete the table in the 'show your work' box.  You must complete EVERY box, not just the colored boxes!

Next, match the colored boxes with the number that you wrote in the box.

anion

2+

79

36

80

cation

22

10

19

What charge do group 1 elements form when they form ions?

2+

1+

0

1-

2-

What charge do group 2 elements form when they form ions?

2+

1+

0

1-

2-

What charge do group 13 elements form when they form ions?

3+

2+

0

2-

3-

What charge do group 15 elements form when they form ions?

3+

2+

0

2-

3-

What charge do group 16 elements form when they form ions?

2+

1+

0

1-

2-

What charge do group 17 elements form when they form ions?

2+

1+

0

1-

2-

4.1 - Ions

4.1 - Ions

Ions

Using what you learned from the simulation, define the term 'ion' in your own words.

Think about your answer to the previous question. Why do you think lithium always forms a +1 ion, beryllium always forms a +2 ion, and boron always forms a +3 ion?

Think about your to the previous question. Why do you think fluorine always forms a -1 ion, oxygen always forms a -2 ion, and nitrogen always forms a -3 ion?

Using a Periodic Table, fill in the table in the "Show Your Work" box to demonstate how the ions listed form. If you are not sure how to fill in the chart, check out this video! Note: You do not need to draw the protons, you can just write the number of protons in the nucleus!

The animation below shows the steps involved in forming an ionic bond. (We'll be learning about these next!!)Analyze the animation below. How are ions that form ionic bonds held together?

Explain why an ionic bond typically forms between a metal and a nonmetal.

Ions

What is the difference between a neutral atom and an ion?

Using what you learned from the simulation, define the term 'ion' in your own words.

What do you notice about the number of electrons in Li1+, Be+2, B3+, and He?

Think about your answer to the previous question. Why do you think lithium always forms a +1 ion, beryllium always forms a +2 ion, and boron always forms a +3 ion?

What do you notice about the number of electrons in F1-, O2-, N3-, and Ne?

Think about your to the previous question. Why do you think fluorine always forms a -1 ion, oxygen always forms a -2 ion, and nitrogen always forms a -3 ion?

Using a Periodic Table, fill in the table in the "Show Your Work" box to demonstate how the ions listed form. If you are not sure how to fill in the chart, check out this video! Note: You do not need to draw the protons, you can just write the number of protons in the nucleus!

Consider the ions you analyzed in the previous question. How could you calculate the charge of an ion?THINK! Focus on one of the ions from the previous question and use the formulas below to calculate the charge. The formula that equals the correct charge is the correct formula.

Notice that you were not asked to determine the charges of ions formed with elements in Group 14. Why do you think this is?

Notice that you were not asked to determine the charges of ions formed with elements in Group 18. Why do you think this is?

Elements in groups 1, 2, and 13 often form cations, while elements in groups 15, 16, and 17 often form anions. Considering this, which of the following are the best definitions for cation and anion?

Consider what you learned in the last lesson about metals and nonmetals.Which of the following statements about ions is correct?

First, complete the table in the 'show your work' box. You must complete EVERY box, not just the colored boxes!Next, match the colored boxes with the number that you wrote in the box.

The animation below shows the steps involved in forming an ionic bond. (We'll be learning about these next!!)Analyze the animation below. How are ions that form ionic bonds held together?

Explain why an ionic bond typically forms between a metal and a nonmetal.

What charge do group 1 elements form when they form ions?

What charge do group 2 elements form when they form ions?

What charge do group 13 elements form when they form ions?

What charge do group 15 elements form when they form ions?

What charge do group 16 elements form when they form ions?

What charge do group 17 elements form when they form ions?

Notice that you were not asked to determine the charges of ions formed with elements in Group 14. Why do you think this is?

Notice that you were not asked to determine the charges of ions formed with elements in Group 18. Why do you think this is?

Using a Periodic Table, fill in the table in the "Show Your Work" box to demonstate how the ions listed form.

If you are not sure how to fill in the chart, check out this video!

Note: You do not need to draw the protons, you can just write the number of protons in the nucleus!

The animation below shows the steps involved in forming an ionic bond. (We'll be learning about these next!!)

Analyze the animation below. How are ions that form ionic bonds held together?

Using a Periodic Table, fill in the table in the "Show Your Work" box to demonstate how the ions listed form.

If you are not sure how to fill in the chart, check out this video!

Note: You do not need to draw the protons, you can just write the number of protons in the nucleus!

Consider the ions you analyzed in the previous question. How could you calculate the charge of an ion?

THINK! Focus on one of the ions from the previous question and use the formulas below to calculate the charge. The formula that equals the correct charge is the correct formula.

Consider what you learned in the last lesson about metals and nonmetals.

Which of the following statements about ions is correct?

First, complete the table in the 'show your work' box. You must complete EVERY box, not just the colored boxes!

Next, match the colored boxes with the number that you wrote in the box.

The animation below shows the steps involved in forming an ionic bond. (We'll be learning about these next!!)

Analyze the animation below. How are ions that form ionic bonds held together?