Sodium (Na) has an ionization energy of 495 kJ/mol. Chlorine (Cl) has an ionization energy of 1251 kJ/mol. Which of the following is a possible explanation for the trend?

Chlorine has stronger attractive forces between the nucleus and the electrons due to an increase in the effective nuclear force (pull). It takes more energy to remove an electron from chlorine than sodium.

Ionization energy increases down the periodic table and decreases across the periodic table.

Sodium has a smaller atomic radius than chlorine. It takes less energy for an electron to be added to the outer energy level on sodium than the outer energy level on chlorine.

Chlorine has weaker attractive forces between the nucleus and the electrons due to an increase in shielding. It takes more energy to remove an electron from chlorine than sodium.

As you move across the periodic table from left to right, the atomic radius decreases. This is because -

the number of protons increases causing the effective nuclear charge (pull) to increase.

the number of shielding decreases causing the effective nuclear charge (pull) to increase.

the number of electrons increases

Francium (Fr) has the lowest ionization energy in Group 1 because -

its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

it has the smallest number of valence electrons

it has the greatest atomic mass

it has the greatest number of protons, so it attracts its electrons the strongest

The second ionization energy for any element is always higher than the first ionization energy, because -

the nuclear attraction becomes stronger with every electron removed

the number of energy levels increases with every electron removed

the electron repulsion increases with every electron removed

the number of neutrons increases with every electron removed

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 when bonded.

Which atomic trend does the periodic table above show? The arrow points to increasing.

Ionization and Electronegativity

Electronegativity and Atomic Radius

Francium (Fr) has the lowest ionization energy in Group 1 because -

its 1 valence electron is very far from the nucleus, so a low amount energy is needed to remove it

it has the smallest number of valence electrons

it has the greatest atomic mass

it has the greatest number of protons, so it attracts its electrons the strongest

Electrons Configurations & Periodic Trends

Authored by Sonia Rodriguez

Chemistry

9th - 12th Grade

NGSS covered

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Electrons Configurations & Periodic Trends

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MULTIPLE CHOICE QUESTION

45 sec • 1 pt

Which electron configuration represents an an element with 6 valence electrons?

1s²2s²2p²

1s²2s²2p⁶

1s²2s²2p⁴

1s²2s²2p⁴3s²

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

1 min • 1 pt

What charge will an Oxygen ion have?

-1

-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following will have a larger radius than Zinc?

Gallium (Ga)

Aluminum (Al)

Magnesium (Mg)

Strontium (Sr)

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following will have a lower ionization energy than Scandium (Sc)?

Helium (He)

Titanium (Ti)

Calcium (Ca)

Bromine (Br)

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

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.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which electron configuration belongs to Copper (Cu)?

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4d⁸

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4d⁹

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁹

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is this element?
[Ne] 3s²3p⁶4s²

Calcium

Sodium

Scandium

Titanium

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

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Electrons Configurations & Periodic Trends

Which electron configuration represents an an element with 6 valence electrons?

What charge will an Oxygen ion have?

Which of the following will have a larger radius than Zinc?

Which of the following will have a lower ionization energy than Scandium (Sc)?

Which statement correctly and completely identifies a trend?

Which electron configuration belongs to Copper (Cu)?

What is this element?
[Ne] 3s²3p⁶4s²

Put these in increasing of electronegativity order:
F, N, B

What element in period 2 has 7 valence electrons?

What is the attraction of electrons from one element to another when bonded?

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Electrons Configurations & Periodic Trends

Which electron configuration represents an an element with 6 valence electrons?

What charge will an Oxygen ion have?

Which of the following will have a larger radius than Zinc?

Which of the following will have a lower ionization energy than Scandium (Sc)?

Which statement correctly and completely identifies a trend?

Which electron configuration belongs to Copper (Cu)?

What is this element? [Ne] 3s23p64s2

Put these in increasing of electronegativity order:F, N, B

What element in period 2 has 7 valence electrons?

What is the attraction of electrons from one element to another when bonded?

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Popular Resources on Wayground

Discover more resources for Chemistry

What is this element?
[Ne] 3s²3p⁶4s²

Put these in increasing of electronegativity order:
F, N, B