Understanding Titanium: Isotopes and Properties

This video tutorial explains how to determine the atomic number, protons, neutrons, electrons, and mass number for titanium. It covers the concept of isotopes, focusing on titanium's naturally occurring isotopes and their respective neutron counts. The video also discusses how to calculate the number of neutrons using the mass number and highlights the significance of the average atomic mass. The tutorial emphasizes that titanium is neutral, meaning its protons and electrons are equal, and provides practical examples to illustrate these concepts.

What is the atomic number of titanium?

• 21

• 22

• 20

• 23

How many protons are present in all isotopes of titanium?

• 20

• 21

• 22

• 23

Why is titanium considered neutral?

• It has no protons.

• It has more electrons than protons.

• It has an equal number of protons and electrons.

• It has more protons than electrons.

If a titanium isotope has a mass number of 46, how many neutrons does it have?

• 28

• 26

• 24

• 22

For titanium-47, how many neutrons are present?

• 23

• 24

• 25

• 26

What is the mass number of titanium-46?

• 44

• 45

• 47

• 46

What percentage of naturally occurring titanium is titanium-48?

• 50%

• 60%

• 80%

• 73%

How is the average atomic mass of titanium calculated?

• By considering the abundance and mass numbers of all isotopes.

• By using only the mass number of titanium-48.

• By averaging the mass numbers of the most abundant isotopes.

• By adding the mass numbers of all isotopes.

Which of the following is true about isotopes of titanium?

• They have different atomic numbers.

• They have the same number of neutrons.

• They have the same number of protons.

• They have different numbers of electrons.

What should you do if you are not given the mass number or neutrons for an element?

• Use the mass number of the most common isotope.

• Look at the periodic table and round the average atomic mass.

• Use the atomic number.

• Guess the values.