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

Authored by Jerry Morton

Chemistry

10th - 12th Grade

NGSS covered

Used 192+ times

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N^3-

O^2-

F^-

Na⁺

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which of the following is the smallest in size?

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What atom matches this electron configuration?
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When an atom loses a valence electron, it becomes a(n) _____________ ion.

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