distinguishing among atoms

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Distinguishing Among Atoms

Just as apples come in different varieties, a chemical element can come in different “varieties” called isotopes.

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Distinguishing Among Atoms >

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4.3 Atomic Number

Atomic Number

What makes one element different from another?



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4.3 Atomic Number

Elements are different because they contain different numbers of protons.

The atomic number of an element is the number of protons in the nucleus of an atom of that element.


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Atomic Number


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Practice Problems for Conceptual Problem 4.1

Problem Solving 4.15 Solve Problem 15 with the help of an interactive guided tutorial.



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Mass Number

Mass Number

How do you find the number of neutrons in an atom?

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>Distinguishing Among Atoms Mass Number

The total number of protons and neutrons in an atom is called the mass number.

The number of neutrons in an atom is the difference between the mass number and atomic number.

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>Distinguishing Among Atoms Mass Number

Au is the chemical symbol for gold.

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SAMPLE PROBLEM

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Practice Problems for Sample Problem 4.1




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Isotopes

Isotopes

How do isotopes of an element differ?

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>Distinguishing Among Atoms4.3 Isotopes

Isotopes are atoms that have the same number of protons but different numbers of neutrons.

Because isotopes of an element have different numbers of neutrons, they also have different mass numbers.

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>Distinguishing Among Atoms Isotopes

Despite these differences, isotopes are chemically alike because they have identical numbers of protons and electrons.

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Practice Problems for Conceptual Problem 4.2

Problem Solving 4.20Solve Problem 20 with the help of an interactive guided tutorial.



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Atomic Mass

Atomic Mass

How do you calculate the atomic mass of an element?

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>Distinguishing Among Atoms Atomic Mass

Measurement unit for Atomic mass = An atomic mass unit (amu) is defined as one twelfth of the mass of a carbon-12 atom.

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The atomic mass of an element is a weighted average mass of the atoms in a naturally occurring sample of the element.

A weighted average mass reflects both the mass and the relative abundance of the isotopes as they occur in nature.

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Practice Problems

for Conceptual Problem 4.3


for Conceptual Problem 4.3



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Atomic Mass

To calculate the atomic mass of an element, multiply the mass of each isotope by its natural abundance, expressed as a decimal, and then add the products.

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For example, carbon has two stable isotopes:

• Carbon-12, which has a natural abundance of 98.89%, and

• Carbon-13, which has a natural abundance of 1.11%.

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SAMPLE PROBLEM

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SAMPLE PROBLEM

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SAMPLE PROBLEM

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SAMPLE PROBLEM

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Practice Problems for Sample Problem 4.2




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The Periodic Table—A Preview

The Periodic Table—A Preview

Why is a periodic table useful?

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>Distinguishing Among Atoms The Periodic Table—A Preview

A periodic table is an arrangement of elements in which the elements are separated into groups based on a set of repeating properties.

A periodic table allows you to easily compare the properties of one element (or a group of elements) to another element (or group of elements).

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The Periodic Table

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• Each horizontal row of the periodic table is called a period.

• Within a given period, the properties of the elements vary as you move across it from element to element.

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A Period

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• Each vertical column of the periodic table is called a group, or family.

• Elements within a group have similar chemical and physical properties.

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A Group or Family

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Section Quiz

-or-Continue to: Launch:

Assess students’ understanding of the concepts in Section

4.3 Section Quiz

4.3.


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4.3 Section Quiz

1. Isotopes of an element have

a. the same mass number.

b. different atomic numbers.

c. the same number of protons but different numbers of neutrons.

d. the same number of protons but different numbers of electrons.


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4.3 Section Quiz

2. How many neutrons are in sulfur-33?

a. 16 neutrons

b. 33 neutrons

c. 17 neutrons

d. 32.06 neutrons


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4.3 Section Quiz

3. If sulfur contained 90.0% sulfur-32 and 10.0% sulfur-34, its atomic mass would be

a. 32.2 amu.

b. 32.4 amu.

c. 33.0 amu.

d. 35.4 amu.

END OF SHOW

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