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

The atoms have more energy levels

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

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.

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

What are the two variables that affect Coulombic Attraction?

Distance between charges and amount of charge

Number of neutrons and number of protons

Number of neutrons and number of electrons

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.

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.

Na + and Mg 2+ are isoelectronic. Which one will be smaller in radius, and why?

Mg 2+ , because it has more protons and greater effective nuclear charge

Mg 2+ , because it has less electrons and greater repulsion between them

Na + , because it has less electrons and a weaker shielding effect

Na + , because it has more protons and a stronger shielding effect

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

its valence electron is well shielded, so it feels little Coulombic attraction to the nucleus

it has the smallest number of valence electrons

it has the greatest atomic mass

it has the greatest effective nuclear charge, so it feels little Coulombic attraction to the nucleus

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

After you take the last electron in a shell (energy level), the ionization energy to remove the next electron increases dramatically because -

the Coulombic attraction increases dramatically, since the next electron is closer to the nucleus

the Coulombic attraction decreases dramatically, since the next electron is closer to the nucleus

the repulsion between electrons is increased

the number of protons decreases

Chlorine and Fluorine are both very electronegative, as they are both missing a single electron from their valence energy level. Why is Fluorine more electronegative than Chlorine?

Fluorine has less energy levels.

Chlorine has more electrons in its outer shell

The data table below shows atomic radii and Coulombic attraction for four elements. What is the best conclusion that would be supported by this data?

Larger atoms attract electrons more weakly

Atomic radius and Coulombic attraction are unrelated

Atoms with a larger mass have smaller radius

Larger atoms attract electrons more strongly

The graph shows atomic radii of the noble gases. Explain the reason for the trend observed.

Atomic radius is increasing because there are more energy levels.

Atomic radius is increasing because the nuclear charge is increasing.

Atomic radius is increasing because there is a greater attraction of electrons towards the nucleus.

Atomic radius is increasing because these elements are noble gases.

Which of the following is true about a sulfur atom and a chlorine atom?

Sulfur is larger and has lower ionization energy.

Sulfur is larger and has higher ionization energy.

Sulfur is smaller and has higher ionization energy.

Sulfur is smaller and has lower ionization energy.

1U5 Periodic Trends

Authored by Carol Grant

Chemistry

10th Grade

NGSS covered

Used 9+ times

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which has the greater electronegativity:
Cl or Al?

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which has the greater electronegativity:
N or C?

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which has the greater electronegativity:
H or F?

MULTIPLE CHOICE QUESTION

1 min • 14 pts

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

Gallium

Aluminum

Magnesium

Strontium

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

1 min • 14 pts

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

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....

decreases

increases

remains the same

none of the above

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

1 min • 14 pts

Which atom has the largest atomic radius?

potassium

rubidium

francium

cesium

Tags

NGSS.HS-PS1-1

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1U5 Periodic Trends

Which has the greater electronegativity: Cl or Al?

Which has the greater electronegativity: N or C?

Which has the greater electronegativity: H or F?

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

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

As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....

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, ______________.

Atoms that have a high electronegativity, _______________.

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Which has the greater electronegativity:
Cl or Al?

Which has the greater electronegativity:
N or C?

Which has the greater electronegativity:
H or F?