Atomic Theory Review

Atomic Theory Review

11th Grade

23 Qs

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 Atomic Theory Review

Atomic Theory Review

Assessment

Quiz

Mathematics

11th Grade

Practice Problem

Medium

Created by

Aniyah EastWakeHS

Used 2+ times

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23 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

45 sec • 1 pt

Which conclusion was a direct result of the gold foil experiment?

An atom is mostly empty space with a dense, positively charged nucleus.

An electron has properties of both waves and particles.

An atom is composed of at least three types of subatomic particles.

An electron has a positive charge and is located inside the nucleus.

2.

MULTIPLE CHOICE QUESTION

45 sec • 1 pt

The major portion of an atom’s mass is made up of:

Electrons and protons

Neutrons and protons

Neutrons and positrons

Electrons and neutrons

3.

MULTIPLE CHOICE QUESTION

45 sec • 1 pt

Which subatomic particle has no charge?

Alpha particle

Electron

Beta particle

Neutron

4.

MULTIPLE CHOICE QUESTION

45 sec • 1 pt

What is the structure of a krypton-85 atom?

36 electrons, 36 protons, and 49 neutrons

49 electrons, 49 protons, and 85 neutrons

36 electrons, 36 protons, and 84 neutrons

49 electrons, 49 protons, and 49 neutrons

5.

MULTIPLE CHOICE QUESTION

45 sec • 1 pt

Which statement about an atom identifies the element?

The sum of the number of protons and neutrons in the atom is 3.

The difference between the number of neutrons and protons in the atom is 1.

The atom has 1 proton.

The atom has 2 neutrons.

6.

MULTIPLE CHOICE QUESTION

45 sec • 1 pt

Which statement describes the distribution of charge in an atom?

A neutral nucleus is surrounded by one or more positively charged electrons.

A positively charged nucleus is surrounded by one or more negatively charged electrons.

A neutral nucleus is surrounded by one or more negatively charged electrons.

A positively charged nucleus is surrounded by one or more positively charged electrons.

7.

MULTIPLE CHOICE QUESTION

45 sec • 1 pt

The weighted average of the atomic masses of the naturally occurring isotopes of an element is called the:

Formula mass of each isotope

Mass number of each isotope

Atomic number of the element

Atomic mass of the element

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