Honors Chemistry 1.1 Study Guide

Front

What is the average atomic mass of an element with isotopes of 75.23 amu (24.1% abundance), 74.61 amu (48.7% abundance), and 75.20 amu (27.2% abundance)?

Back

74.92 amu

Front

Calculate the average atomic mass of an element with isotopes of 10.013 amu (19.9% abundance) and 11.01 amu (80.1% abundance). What element is it?

Back

10.812, Boron

Front

Define matter.

Back

Matter is anything that has mass and occupies space.

Front

Define energy.

Back

Energy is the ability to do work.

Front

What is the difference between matter and energy?

Back

Matter has mass and occupies space; energy is the ability to do work.

Front

What is the formula to calculate average atomic mass based on isotopic abundance?

Back

Average Atomic Mass = (mass1 * abundance1) + (mass2 * abundance2) + ...

Front

What is the significance of isotopes in chemistry?

Back

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons, affecting their mass.

Front

What is the unit of atomic mass?

Back

Atomic mass is measured in atomic mass units (amu).

Front

What does it mean if an element has a higher average atomic mass?

Back

It indicates that the element has a greater proportion of heavier isotopes.

Front

What is the relationship between mass and energy according to Einstein's theory?

Back

Mass and energy are interchangeable, as expressed in the equation E=mc².