Which has the greater EN: N or C?

N because nitrogen would gain 3 electrons to become stable it has a greater electronegativity.

C because carbon would gain 4 electrons to become stable it has a greater electronegativity.

Which has the greater EN: H or F?

F because fluorine has a -1 charge that means it would gain one electron.

H because hydrogen has a +1 charge that means it would gain one electron.

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

Strontium because it has more energy levels therefore it has more shielding electrons making the atom larger.

Gallium because as you go across the row the nuclear charge decreases so the size of the atom increases.

Aluminum because as you go across the row the nuclear charge increases so the size of the atom increases.

Magnesium because it has more energy levels therefore it has more shielding electrons making the atom larger.

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

Nitrogen (N) because it has a smaller atomic radius so valence electrons are closer to the nucleus making it more difficult to remove an electron.

Iodine because smaller atomic radius so valence electrons are closer to the nucleus making it more difficult to remove an electron.

Antimony (Sb) because it has a larger atomic radius than As so it is valence electrons are further from the nucleus so more energy is required to remove an electron.

Germanium (Ge) because it has a larger atomic radius than As so it is valence electrons are further from the nucleus so more energy is required to remove an electron.

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, ______________.

the atoms have more protons creating a stronger force of attraction between the protons and electrons.

the atoms have more neutrons creating a stronger force of attraction between the nucleus and electrons.

the atoms have less mass so the size would decrease.

the atoms have less electrons creating a stronger force of attraction between the protons and electrons.

Electronegativity is how good an atom is at attracting electrons. Therefore which of the following statements is correct?

Non metals are more electronegative because they are anions and want to gain electrons.

Non metals are more electronegative because they are cations and want to gain electrons.

Non metals are more electronegative because they are anions and want to lose electrons.

Non metals are more electronegative because they are cations and want to lose electrons.

Which element is more reactive: K or CS?

Cs because it has a larger atomic radius and valence electrons are further from the nucleus making it more reactive.

K because it has a smaller atomic radius and valence electrons are held more tightly making it more reactive.

Cs because it has a smaller atomic radius and valence electrons are held more tightly making it more reactive.

K because it has a larger atomic radius and valence electrons are further from the nucleus making it more reactive.

Which are the most stable elements on the periodic table?

Noble gases because they have 8 valence electrons.

Alkali Metals because they have 1 valence electron.

Halogens because they have 1 valence electron.

Carbon Family because they have 4 valence electrons.

Which group of elements would have similar chemical properties?

N, P, AS because they are in the same family and have the same number of valence electrons they would be chemically similar.

Na, MG, Al because they are in the same period they would be chemically similar.

Fr, Ba, Y because they are all metals in the same family they would be chemically similar.

H, O, N because they are all non-metals they would be chemically similar.

Compare an atoms first ionization energy with the second ionization energy, which is higher?

The first ionization energy is lower because it takes less energy to remove an electron from a neutral atom than it does from a positively charged atom.

The first ionization energy is greater because it takes more energy to remove an electron from a neutral atom than a positively charged atom.

The second ionization energy is greater because it takes more energy to remove an electron from a neutral atom than it does from a positively charged atom.

The second ionization energy is less because it takes less energy to remove an electron from a positively charged atom than a neutral atom.

Why would there be no reaction between sodium and Gallium?

Both elements are metals that become stable by losing valence electrons.

Both elements are non metals that become stable by gaining valence electrons.

Both elements are non metals that become stable by losing valence electrons.

Both elements are metal that become stable by gaining valence electrons.

Which statement is correct concerning the trend for atomic radius?

Across a period atoms get smaller because additional protons increase the force of attraction between the nucleus and the electrons. Down a group atoms get bigger because of the addition of energy levels results in an increased number of shielding electrons between the nucleus and valence electrons.

Across a period atoms get bigger because additional protons decrease the force of attraction between the nucleus and the electrons. Down a group atoms get smaller because of the addition of energy levels resulting in a stronger attraction between nucleus and electrons.

Across a period atoms get bigger because additional protons decrease the force of attraction between the nucleus and the electrons. Down a group atoms get bigger because of the addition of energy levels results in an increased number of shielding electrons between the nucleus and valence electrons.

Across a period atoms get bigger because additional protons decrease the force of attraction between the nucleus and the electrons. Down a group atoms get smaller because of the addition of energy levels results in an increased number of shielding electrons between the nucleus and valence electrons resulting in a stronger attraction.

Elements J and K are compared. Element K has a larger atomic radius than Element J. Based on this, what conclusion can be drawn?

Element K is located closer to the bottom left than Element J.

Element K is located closer toward the top right of the peroidic table than Element J.

Element K is located closer to the top of the periodic table than Element J.

Element K is located closer to the bottom right than Element J.

Periodic Trends

Authored by Jennifer Lucky

Chemistry

10th - 12th Grade

NGSS covered

Used 30+ times

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30 questions

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MULTIPLE CHOICE QUESTION

2 mins • 1 pt

A measure of the size of an atom, and is generally defined as the distance from the nucleus to the outermost electron orbit

chemical reactivity

atomic radius

energy levels

orbit

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

The core of an atom where most of the mass of an atom exists; contains protons and neutrons

nucleus

electron shell

proton

electron

Tags

NGSS.HS-PS1-8

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

The minimum energy required to remove an electron from the ground state of an atom

electron configuration

energy levels

ionization energy

ionic bond

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

The tendency of an atom to attract electrons and acquire a negative charge

electronegativity

charge

bonding ability

electron configuration

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Vertical columns of elements (families) on the periodic table with similar valence electron configurations and similar properties

groups

periods

quadrants

rows

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

An electron that resides in the outermost shell, or principal quantum level, of an atom

periodic trend

electron shell

ionic radius

valence electron

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Which has the greater EN:
Cl or Al?

Cl because it is an anion that would gain electrons.

Al because it is a cation that would gain electrons.

Tags

NGSS.HS-PS1-1

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Periodic Trends

A measure of the size of an atom, and is generally defined as the distance from the nucleus to the outermost electron orbit

The core of an atom where most of the mass of an atom exists; contains protons and neutrons

The minimum energy required to remove an electron from the ground state of an atom

The tendency of an atom to attract electrons and acquire a negative charge

Vertical columns of elements (families) on the periodic table with similar valence electron configurations and similar properties

An electron that resides in the outermost shell, or principal quantum level, of an atom

Which has the greater EN: Cl or Al?

Which has the greater EN: N or C?

Which has the greater EN: H or F?

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

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Which has the greater EN:
Cl or Al?

Which has the greater EN:
N or C?

Which has the greater EN:
H or F?