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

The atoms have more energy levels

As you move across the periodic table atoms tend to get smaller because, ______________.

effective nuclear charge tends to increase

the atoms have more mass, which increases the gravitational pull

it doesn't, atoms get bigger going from left to right because of the additional protons and electrons that are being added.

atoms lose energy levels make them smaller

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

Metals have the largest -

atomic radius and electronegativity

electronegativity and ionization energy

ionization energy and atomic radius

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.

The electronegativity of Cl is the highest in Period 2. Why?

Cl is the smallest and has the greatest effective nuclear charge

Cl is the largest and has the greatest effective nuclear charge

Cl is the smallest and has the lowest effective nuclear charge

Cl is the largest and has the lowest effective nuclear charge

Atomic radius generally increases as we move __________.

down a group and from right to left across a period

up a group and from left to right across a period

down a group and from left to right across a period

up a group and from right to left across a period

When looking at elements in the same period, why does increasing the effective nuclear charge make the atoms smaller?

It increases the force of attraction on the valence electrons thus pulling the electrons closer to the nucleus and making the atom smaller

It increases the force of attraction between the protons thus pulling the protons closer together and making the atom smaller

If reduces the number of main energy levels or shells thus making the atom smaller

It increases the force of repulsion the electrons have on each other thus causing the electrons to spread out and making the atom smaller

Why are cations smaller than their parent atoms?

when cations form they lose electrons which reduces the repulsion force between the electrons allowing the electron cloud to shrink.

when cations form they gain protons which increases the effective nuclear charge which increases the force of attraction of the nucleus on the electrons causing the electron cloud to shrink

Why are anions larger than their parent atoms?

when anions form they gain electrons which increases the repulsion force between the electrons causing the electron cloud to expand.

when anions form they gain an additional outer shell thus making them larger

The electron cloud is ... (pick all that apply)

mostly electrons with little empty space

static (does NOT change its size)

C02 Trends of the Periodic Table

10th - 11th Grade

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145 Qs

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C02 Trends of the Periodic Table

Quiz

•

Chemistry

•

10th - 11th Grade

•

Practice Problem

•

Medium

•

NGSS

HS-PS1-1, HS-PS1-2, HS-PS2-5

Standards-aligned

Bill Habiger

Used 15+ times

FREE Resource

145 questions

Show all answers

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Base on the trend, which has the greater electronegativity,
Cl or Al?

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Base on the trend, which has the greater electronegativity,
N or C?

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Based on the trend, which has the greater electronegativity,
H or F?

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

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

Gallium

Aluminum

Magnesium

Strontium

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Which of the following will have a higher electronegativity than arsenic (As)?

Carbon (C)

Neon (Ne)

Antimony (Sb)

Germanium (Ge)

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

1 min • 1 pt

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

Helium (He)

Titanium (Ti)

Calcium (Ca)

Magnesium (Mg)

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

1 min • 1 pt

For elements in Group 16, how does the electronegativity change as you go down the group?

decreases

increases

remains the same

none of the above

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C02 Trends of the Periodic Table

145 questions

Base on the trend, which has the greater electronegativity,Cl or Al?

Base on the trend, which has the greater electronegativity,N or C?

Based on the trend, which has the greater electronegativity, H or F?

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

Which of the following will have a higher electronegativity than arsenic (As)?

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

For elements in Group 16, how does the electronegativity change as you go down the group?

Which atom has the largest atomic radius?

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

As you move across the periodic table atoms tend to get smaller because, ______________.

Create a free account and access millions of resources

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Discover more resources for Chemistry

Base on the trend, which has the greater electronegativity,
Cl or Al?

Base on the trend, which has the greater electronegativity,
N or C?

Based on the trend, which has the greater electronegativity,
H or F?