Anatomy Unit 2 Study Guide

Unit 2 Lecture Study Guide

1) What are the parts of an atom? Where are the subatomic particles found?

The three subatomic particles in an atom are protons, neutrons, and electrons.

1) Protons have a relative mass of 1 and a charge of +1, and they are found in the nucleus of an atom.

2) Neutrons have a relative mass of 1 and no charge, and they are also found in the nucleus of an atom.

3) Electrons have a relative mass of 1/1836 and a charge of -1. They are found in specific orbits around the nucleus and are held in these orbits by the positive charge of the protons in the nucleus.

2) How does the Atomic Mass # differ from the Atomic #?

Atomic mass is also known as atomic weight. Atomic mass is the weighted average mass of an atom of an element based on the relative natural abundance of that element's isotopes.

Mass number is a count of the total number of protons and neutrons in an atom's nucleus.

3) What is an isotope? Give an example (show how it is an isotope).

Isotopes are variants of a particular chemical element. While all isotopes of a given element share the same number of protons, each isotope differs from the others in its number of neutrons. For example, carbon-12, carbon-13 and carbon-14 are three isotopes of the element carbon with mass numbers 12, 13 and 14. The atomic number of carbon is 6 which mean that every carbon atom has 6 protons, so that the neutron numbers of these isotopes are 6, 7 and 8.

4) Compare and contrast the 3 basic types of chemical bonds and give an example of each.

An ionic bond is an electrostatic interaction between atoms that have a huge electronegative difference. An ionic bond is formed when an atom accepts or donates one or more valence electrons to another atom. A negative ion (Anion) and a positive ion (Cation) are formed during the chemical ionic bonding. An example is Sodium and fluorine bonding ionically to form sodium fluoride.

A Covalent bond...