What are the two variables that affect Coulombic Attraction?

Number of neutrons and number of protons

Number of neutrons and number of electrons

Distance and number of neutrons

What is the trend in Coulombic attraction moving from left to right across a period?

Coulombic attraction increases moving from left to right across a period.

Coulombic attraction decreases moving from left to right across a period.

The trend depends upon which period is being observed.

What is the trend in Coulombic attraction going down a group?

Coulombic attraction decreases moving down a group.

Coulombic attraction increases moving down a group.

The trend depends upon which group is being observed.

Ionization energy is the...

energy needed to remove the outermost electron.

ability of an atom to attract electrons from another atom.

Electronegativity is the...

ability of an atom to attract electrons from another atom.

energy needed to remove the outermost electron.

As you move down a group, atomic radius increases because -

you add more and more shells (energy levels)

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

the number of protons increases, so attraction to electrons increases

the number of energy levels increases

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

Electronegativity is...

the ability of an atom to attract/ accept 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.

Practice Quiz- Coulombic Attraction & Valence Trends

9th - 11th Grade

•

38 Qs

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Practice Quiz- Coulombic Attraction & Valence Trends

Quiz

•

Chemistry

•

9th - 11th Grade

•

Practice Problem

•

Medium

•

NGSS

HS-PS1-1, HS-PS2-4, MS-PS1-1

Standards-aligned

Justin Foley

Used 86+ times

FREE Resource

38 questions

Show all answers

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which is most likely to form a negative ion?

an element from group 17

a metal

an element from group 1

an element with atoms that have eight valence electrons

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

1 min • 1 pt

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

positive

negative

neutral

polyatomic

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

An atom of which element is represented in the following Bohr model?

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How many valence electrons does a neutral atom of sulfur contain?

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How many protons, neutrons, and electrons does a neutral atom of nitrogen have?

P = 7, N = 14, E = 7

P = 7, N = 7, E = 7

P = 7, N =14, E = 14

P = 14, N = 14, E = 14

Tags

NGSS.MS-PS1-1

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Based on its position in the periodic table, which element has 7 electrons in its highest energy level while at ground state?

nitrogen (N)

chlorine (Cl)

rubidium (Rb)

manganese (Mn)

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

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Practice Quiz- Coulombic Attraction & Valence Trends

38 questions

Which is most likely to form a negative ion?

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

An atom of which element is represented in the following Bohr model?

How many valence electrons does a neutral atom of sulfur contain?

How many protons, neutrons, and electrons does a neutral atom of nitrogen have?

Based on its position in the periodic table, which element has 7 electrons in its highest energy level while at ground state?

This is an atom of which element?

If the number of energy level rings remains the same, as the number of protons increases, the force of attraction

As the distance between protons and electrons increases, the force of attraction

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