Valence electrons are defined a the ...........

Electrons farthest away from the nucleus

Electrons closest to the nucleus

Electrons that just come and go - they don't stay with the atom

Select the correct order of waves on the EMS

Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma

Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio

Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio

Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma

Put the visible light colors in order from longest wavelength to shortest wavelength

Red, Orange, Yellow, Green, Blue, Indigo, Violet

Violet, Indigo, Blue, Green, Orange, Yellow, Red

Red, Yellow, Green, Orange, Violet, Blue, Indigo

As you move down the periodic table atoms get bigger. This is because ____________.

The atoms have more energy levels

Atoms that have a high electronegativity, _______________.

hold on to their electrons more tightly.

give up their electrons more easily.

Electronegativity is...

how good an atom is at attracting electrons

the ability of an atom to lose electrons

the energy required to remove an electron from a specific atom

how easy it is to make friends.

Ionization energy is...

how much energy it takes to remove an electron from an atom

the energy required to add an electron to a specific atom

the energy required to shield the outer electrons from the nucleus

a measure of the ability of an atom to attract electrons

Which statement correctly and completely identifies a trend?

Atomic radius decreases across a period and increases down a group.

Electronegativity decreases across a period and decreases down a group.

Ionization energy increases across a period and increases down a group.

Ionic radius increases across a period and increases down a group.

Fluorine (F) has one of the highest ionization energies on the periodic table because -

its electrons are close to and have a very strong attraction to the nucleus

it has seven valence electrons, and just needs one more electron to gain stability

it is one of the largest atoms on the periodic table

The Br - anion is larger than the Br atom because -

Br - has more electrons than Br, and more electrons repel each other

Br has more electrons than Br - , and more electrons repel each other

Br - has more protons, so it has more attraction for its electrons

Br has more protons, so it has more attraction for its electrons

Electronic Structure test review

Quiz

•

Chemistry

•

10th - 12th Grade

•

Practice Problem

•

Medium

•

NGSS

HS-PS1-1, HS-PS4-1, HS-PS1-2

+1

Standards-aligned

Jerry Morton

Used 192+ times

FREE Resource

57 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

N^3-

O^2-

F^-

Na⁺

7.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which of the following is the smallest in size?

K

Na

Li

Cs

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57 questions

The electron configuration of an atom is 1s²2s²2p⁶. The number of electrons in the atom is

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

What is the noble gas shorthand electron for Sulfur atom?

What atom matches this electron configuration?
[Xe] 6s²5d⁹

What electron configuration matches an oxygen atom?

Which of the following is the smallest in size?

Which of the following is the smallest in size?

An orbital can at most hold how many electrons?

When an atom loses a valence electron, it becomes a(n) _____________ ion.

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The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is

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Which of the following is the smallest in size?

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