Atomic Structure and Isotopes

The video tutorial explains how to analyze isotopes and ions by examining subatomic particles. It covers determining the number of protons, neutrons, and electrons, as well as calculating the mass number and charge of atoms. The tutorial uses examples of bromine, mercury, and phosphorus to illustrate these concepts, emphasizing the relationship between atomic number, mass number, and isotopic symbols.

What is the relationship between atomic number and the number of protons in an atom?

• Atomic number is equal to the number of protons.

• Atomic number is unrelated to the number of protons.

• Atomic number is always double the number of protons.

• Atomic number is half the number of protons.

How do you calculate the mass number of an isotope?

• Add the number of protons and neutrons.

• Subtract the number of neutrons from the atomic number.

• Multiply the number of protons by the number of neutrons.

• Add the number of protons and electrons.

Which element has the atomic number 35?

• Fluorine

• Iodine

• Bromine

• Chlorine

What charge does an atom have if it gains one electron?

• Neutral

• Positive two

• Negative one

• Positive one

What is the atomic number of Mercury?

• 82

• 78

• 79

• 80

How many neutrons are in a Mercury isotope with a mass number of 202?

• 118

• 124

• 120

• 122

If a Mercury atom has a +2 charge, how many electrons does it have?

• 80

• 78

• 76

• 82

What is the atomic number of Phosphorus?

• 14

• 16

• 15

• 17

How many neutrons are in a Phosphorus isotope with a mass number of 31?

• 14

• 17

• 16

• 15

What is the charge of a Phosphorus isotope with equal numbers of protons and electrons?

• Double positive

• Neutral

• Negative

• Positive