Which is smaller... Mg or Mg 2+ ?

Mg 2+ because it loses an energy level

Mg because it gains an energy level

Mg due to extra electron repulsion

Mg 2+ because of extra electron repulsion

Why doesn't having more protons increase the attraction down a column?

as energy levels are added, non-valence electrons block the extra protons from attracting ve-

there are more valence electrons in the outermost energy level

actually, there aren't more protons in the nucleus down the column

more neutrons block the extra protons

What happens to atomic radius across a period?

the atoms get smaller because with more attraction to the extra protons, the e- cloud moves closer to the nucleus

the atoms get bigger because the nucleus is bigger as more protons are added

the atoms get bigger because there are more ve-

the atoms get bigger because there are more energy levels

Element Z has more protons than element Y, but both have 4 energy levels. Which statement is true?

Z is smaller and would attract electrons more in a bond

Y is smaller and would attract electrons more in a bond

Y is bigger and would attract electrons more in a bond

Z is bigger and would attract electrons more in a bond

Which of the following lose all their ve- when forming an ion?

depends on how many ve- the element has

Which has a higher electronegativity.. Rb or Sr?

Sr, because with more p+ in its nucleus it attracts e- more

Rb, because with more p+ in its nucleus it attracts e- more

Rb, because with more nrg levels the ve- are closer to/ more attracted to the nucleus

Sr, because with more nrg levels the ve- are closer to/ more attracted to the nucleus

Which has a higher ionization energy.. N or As?

N, because with less nrg levels the ve- are closer to/ more attracted to the nucleus making them harder to remove.

N, because with more p+ in its nucleus it attracts e- more making them harder to remove.

As, because with more p+ in its nucleus it attracts e- more making them harder to remove.

As, because with less nrg levels the ve- are closer to/ more attracted to the nucleus making them harder to remove.

Look at the bohr models of Li and Be. Imagine the first valence electron was already removed from both atoms, and now you are going to remove the second valence electron. The energy required to remove the second valence electron is called second ionization energy. Would lithium or beryllium have a higher second ionization energy ?

Li, because the second valence electron comes from an energy level closer to the nucleus

Li, because it has more protons

Be, because it has more protons

Be, because the second valence electron comes from an energy level closer to the nucleus

Li, because the beryllium has two valence electrons that repel each other

Periodicity - Chemistry

Quiz

•

Chemistry

•

KG - University

•

Practice Problem

•

Hard

•

NGSS

HS-PS1-1, HS-PS1-2

Standards-aligned

Lauren Copus

Used 2K+ times

FREE Resource

20 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The trends on the periodic table are dependent on..

how attracted a valence electron is to the nucleus

how attracted valence electrons are to each other

how attracted a valence electrons is to a non valence electron

how attracted a non valence electron is to the nucleus

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

2.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

What makes a valence electron more attracted to the nucleus?

less distance between the nucleus and having less protons

less distance between the nucleus and having more protons

more distance between the nucleus and having less protons

more distance between the nucleus and having more protons

less distance and having more valence electrons

Tags

NGSS.HS-PS1-2

3.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

What is the tendency of an atom to attract electrons towards itself in a bond?

atomic radius

ionization energy

shielding

Electronegativity

Tags

NGSS.HS-PS1-2

4.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

The higher the ionization energy...

the more attracted the valence electron is to the nucleus so it is harder to remove

the less attracted the valence electron is to the nucleus so it is easier to remove

the more attracted the valence electron is to another electron, so it is harder to remove

the more repelled a valence electron is to another electron, so it is easier to remove

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

5.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Which is larger... P or P^3- ?

P^3- because it gains an energy level

P^3- due to extra electron repulsion

P because it loses an energy level

P because of extra electron repulsion

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

6.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Why does ionization energy decrease going down a group?

Adding more energy levels makes the ve- further from the nucleus so it is easier to remove

There are more valence electrons in the outer shell so the ve- is easier to remove

There are more protons in the nucleus so the ve- is easier to remove

There are less protons in the nucleus so the ve- is easier to remove

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

7.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Why does electronegativity increase across a period?

Adding more energy levels makes the ve- further from the nucleus

There are more valence electrons in the outer shell

There are more protons in the nucleus

There are less protons in the nucleus

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

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Periodicity - Chemistry

20 questions

The trends on the periodic table are dependent on..

What makes a valence electron more attracted to the nucleus?

What is the tendency of an atom to attract electrons towards itself in a bond?

The higher the ionization energy...

Which is larger... P or P^3- ?

Why does ionization energy decrease going down a group?

Why does electronegativity increase across a period?

Which is smaller... Mg or Mg²⁺ ?

List the following in order of weakest to strongest ionization energy.
P, Cs, Co, Sr

List the following from largest to smallest atomic radius.
P, Cs, Co, Sr

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Periodicity - Chemistry

20 questions

The trends on the periodic table are dependent on..

What makes a valence electron more attracted to the nucleus?

What is the tendency of an atom to attract electrons towards itself in a bond?

The higher the ionization energy...

Which is larger... P or P3- ?

Why does ionization energy decrease going down a group?

Why does electronegativity increase across a period?

Which is smaller... Mg or Mg2+ ?

List the following in order of weakest to strongest ionization energy.P, Cs, Co, Sr

List the following from largest to smallest atomic radius.P, Cs, Co, Sr

Create a free account and access millions of resources

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

Which is larger... P or P^3- ?

Which is smaller... Mg or Mg²⁺ ?

List the following in order of weakest to strongest ionization energy.
P, Cs, Co, Sr

List the following from largest to smallest atomic radius.
P, Cs, Co, Sr