What happens when the compound NaCl is formed?

Sodium forms an ion with +2 charge and chlorine forms an ion with −2 charge.

Sodium transfers an electron to chlorine.

Sodium receives two electrons from chlorine.

Sodium forms an ion with −1 charge and chlorine forms an ion with +1 charge.

What happens when the compound HCl is formed?

Hydrogen forms an ion with +1 charge; chlorine forms an ion with −1 charge.

Hydrogen transfers two electrons to chlorine.

Hydrogen receives two electrons from chlorine.

Hydrogen forms an ion with −1 charge; chlorine forms an ion with +1 charge.

What happens when the compound MgO is formed?

Magnesium forms an ion with −1 charge; oxygen forms an ion with +1 charge.

Oxygen transfers two electrons to magnesium.

Oxygen receives two electrons from magnesium.

Magnesium forms an ion with +1 charge; oxygen forms an ion with −1 charge.

Which of these statements best describes the formula unit for a compound made from Mg and Cl?

It is MgCl 2 because the total positive charge on Mg is two.

It is MgCl 2 because the total negative charge on Cl is one.

It is Mg 2 Cl because the total negative charge on Mg is one.

It is Mg 2 Cl because the total positive charge on Mg is two.

What is the formula unit for a compound made from Ca and O?

CaO because the total positive charge on O is one.

CaO 2 because the total negative charge on O is two.

Ca 2 O because the total negative charge on Ca is one.

CaO because the total positive charge on Ca is two.

What is the formula unit for a compound made from Li and Cl?

LiCl because the total negative charge on Cl is one.

LiCl because the total negative charge on Li is two.

Li 2 Cl because the total positive charge on Cl is one.

Li 2 Cl because the total positive charge on Li is two.

What best describes the bonding in a water molecule?

An oxygen atom shares an electron pair with each H atom.

An oxygen atom shares a single electron with each H atom.

An oxygen atom receives an electron from each H atom.

An oxygen atom transfers an electron to each H atom.

What best describes the bonding in a silicon dioxide molecule?

A silicon atom shares two electron pairs with each oxygen atom.

A silicon atom transfers an electron to each oxygen atom.

A silicon atom receives two electrons from each oxygen atom.

A silicon atom shares an electron pair with each oxygen atom.

Which of the following best represents and explains the formula for a compound made from carbon and hydrogen?

CH 4 , because four electron pairs are shared between carbon and hydrogen.

CH 2 , because two electron pairs are shared between carbon and hydrogen.

CH 4 , because each hydrogen contributes four electrons to the bonds.

CH 2 , because each carbon contributes two electrons to the bonds.

Which of the following best represents and explains the formula for a compound made from nitrogen and hydrogen?

NH 3 , because nitrogen forms a single bond with each hydrogen atom.

NH 4 , because nitrogen needs four electrons, and each hydrogen needs one electron.

NH 4 , because nitrogen needs one electron, and each hydrogen needs four electrons.

NH 3 , because nitrogen forms a triple bond with each hydrogen atom.

Which of the following best represents and explains the formula for a compound made from fluorine and hydrogen?

HF, because both fluorine and hydrogen are capable of forming only one covalent bond.

HF, because both fluorine and hydrogen are capable of forming only one ionic bond.

H 2 F, because fluorine is short of two electrons, and hydrogen is short of one electron.

H 2 F, because fluorine is capable of forming one, and hydrogen is capable of forming two covalent bonds.

The boiling point of bromine is 59 °C. Which of the following best predicts the boiling point of iodine monochloride, a polar compound?

Higher than 59 °C because dipole-dipole interactions in iodine monochloride are stronger than dispersion forces in bromine.

Lower than 59 °C because ionic bonding in bromine is stronger than covalent bonding in iodine monochloride.

Lower than 59 °C because dipole-dipole interactions in iodine monochloride are weaker than in bromine.

Higher than 59 °C because ionic bonding in iodine monochloride is stronger than H-bonding in bromine.

The boiling point of chlorine is −34 °C. Which of the following best predicts the boiling point of iodine?

Higher than −34 °C because dispersion forces are stronger in iodine due to a greater number of electrons.

Lower than −34 °C because chlorine is more polar than iodine on account of its higher electronegativity.

Higher than −34 °C because dipole-dipole interactions in iodine are stronger than dispersion forces in chlorine.

Lower than −34 °C because permanent dipoles created in chlorine are stronger than temporary dipoles in iodine.

The boiling point of water (H 2 O) is 100 °C. Which of the following best predicts the boiling point of hydrogen sulfide (H 2 S)?

Lower than 100 °C because hydrogen sulfide has dipole-dipole interactions instead of hydrogen bonding.

Higher than 100 °C because ion dipole interactions in hydrogen sulfide are stronger than hydrogen bonding in water.

Lower than 100 °C because the hydrogen bonding in hydrogen sulfide is weaker than it is in water.

Higher than 100 °C because the size of a sulfur atom is larger than the size of an oxygen atom.

What is the goal of the Lewis Dot Structure?

To show the element's valence electrons & bonding capabilities.

To determine the electron position.

To find the atomic mass of an element.

To search for the number of electrons in an individual atom.

When trying to identify an unknown element, a scientist determines what other elements reacts with chemically. Which property of the unknown element determines the other element it reacts with?

The number of valence electrons in the unknown element

The total number of neutrons in the unknown element

The total number of particles in the nucleus of the unknown element

The number of protons in the nucleus of the unknown element

How do electrons of an element determine that element's reactivity?

If the valence shell has missing electrons it is very reactive to attract or lose more electrons.

If the valence shell has a full ring of electrons it is very reactive because it needs more.

If the valence shell has a full shell of electrons it is very reactive because it is already full.

If the valence shell has missing electrons it is not reactive because it is missing electrons.

Module Three Exam Review

Authored by Kristen Baldonado

Science

9th - 12th Grade

NGSS covered

Used 14+ times

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MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Neon is located in the last group of the periodic table. How many valence electrons does the element neon have?

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Lithium is located in the first group of the periodic table. How many valence electrons does the element lithium have?

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Carbon is located in the fourth tall column of the periodic table. How many valence electrons does the element carbon have?

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Atom A has 10 electrons. Atom B has 18 electrons. Which statement is correct?

A will give up electrons to form bonds.

B will give up electrons to form bonds.

Both A and B will be chemically unreactive.

Both A and B will gain electrons to become stable.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Atom A has 11 electrons. Atom B has 17 electrons. Which statement is correct?

A will give up electrons to form bonds.

B will give up electrons to form bonds.

Both A and B will be chemically unreactive.

Both A and B will gain electrons to become stable.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Atom A has 10 electrons. Atom B has 12 electrons. Which statement is correct?

A will give up electrons to form bonds.

B will give up electrons to form bonds.

Both A and B will be chemically unreactive.

Both A and B will gain electrons to become stable.

FILL IN THE BLANKS QUESTION

15 mins • 1 pt

The electron configuration of an element is shown below.

1s²2s²2p⁶3s¹

Name the group this element belongs to in the periodic table.

(a)

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Module Three Exam Review

Neon is located in the last group of the periodic table. How many valence electrons does the element neon have?

Lithium is located in the first group of the periodic table. How many valence electrons does the element lithium have?

Carbon is located in the fourth tall column of the periodic table. How many valence electrons does the element carbon have?

Atom A has 10 electrons. Atom B has 18 electrons. Which statement is correct?

Atom A has 11 electrons. Atom B has 17 electrons. Which statement is correct?

Atom A has 10 electrons. Atom B has 12 electrons. Which statement is correct?

The electron configuration of an element is shown below.

1s²2s²2p⁶3s¹

Name the group this element belongs to in the periodic table.

(a)

The electron configuration of an element is shown below.

1s²2s²2p⁶3s²3p⁶

Name the group this element belongs to in the periodic table.

(a)

What is the charge on an atom after it gains an electron during the formation of a bond?

What is the charge on an atom after it loses an electron during the formation of a bond?

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Similar Resources on Wayground

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Module Three Exam Review

Neon is located in the last group of the periodic table. How many valence electrons does the element neon have?

Lithium is located in the first group of the periodic table. How many valence electrons does the element lithium have?

Carbon is located in the fourth tall column of the periodic table. How many valence electrons does the element carbon have?

Atom A has 10 electrons. Atom B has 18 electrons. Which statement is correct?

Atom A has 11 electrons. Atom B has 17 electrons. Which statement is correct?

Atom A has 10 electrons. Atom B has 12 electrons. Which statement is correct?

The electron configuration of an element is shown below.1s22s22p63s1Name the group this element belongs to in the periodic table. (a)

The electron configuration of an element is shown below.1s22s22p63s23p6Name the group this element belongs to in the periodic table. (a)

What is the charge on an atom after it gains an electron during the formation of a bond?

What is the charge on an atom after it loses an electron during the formation of a bond?

Access all questions and much more by creating a free account

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Science

The electron configuration of an element is shown below.

1s²2s²2p⁶3s¹

Name the group this element belongs to in the periodic table.

(a)

The electron configuration of an element is shown below.

1s²2s²2p⁶3s²3p⁶

Name the group this element belongs to in the periodic table.

(a)