Periodic Table Trends: Atomic Radius, Ionization, and Electronegativity

Why does the ionic radius increase within a family such as the halogens?

The ionic radius increases as the atomic number increases due to the addition of new electron shells.

Why is the atomic radius of sodium smaller than that of potassium?

Sodium has fewer electron shells, resulting in less shielding.

Why do atoms get smaller as you move across a period?

Atoms get smaller because they are getting closer to the nucleus.

What is the trend for ionization energy across the periodic table?

Ionization energy generally increases across a period.

What is the trend for atomic radius across the periodic table?

Atomic radius generally decreases across a period.

What is the trend for electronegativity across the periodic table?

Electronegativity generally increases across a period.

What is the shielding effect?

The shielding effect is the reduction in effective nuclear charge on the electron cloud, due to the presence of other electrons.

Which has a larger ionization energy: sodium or potassium?

Sodium has the larger ionization energy because ionization energy decreases as you move down a group.

What is the most likely ion for magnesium to become when it is ionized?

Mg²⁺.

How does the ionization energy of a noble gas compare to that of a halogen in the same period?

The ionization energy of a noble gas is higher than that of a halogen.

Arrange phosphorus, oxygen, and germanium in order of increasing electronegativity.

Germanium, Phosphorus, Oxygen.

Will the electronegativity of barium be larger or smaller than that of strontium?

Smaller, because electronegativity decreases as you move down a group.

Will the electronegativity of iodine be larger or smaller than that of antimony?

Larger, because iodine has more protons, increasing the nuclear charge.

What is the energy needed to remove the most loosely held electron from a neutral atom called?

First ionization energy.

What is the distance from the nucleus to the outermost electron known as?

Atomic radius.

What is the classification of an element with a high ionization energy?

Nonmetals.

What is the trend for ionization energy as you move down a group?

Ionization energy decreases.

Which atom has the greater nuclear charge: Na or Al?

Aluminum (Al) has a greater nuclear charge.

Which element has the lowest ionization energy?

Cesium or francium.

Which element has the highest electronegativity?

Fluorine.

Which element has the highest ionization energy?

Helium.

Which element has the largest atomic radius?

Cesium or francium.

What is the relationship between the ionic radius of a cation and its atomic radius?

The ionic radius of a cation is smaller than the atomic radius.

Why are noble gases inert and do not form ions?

They have a full outer shell.

Why do elements in the same family generally have similar properties?

They have the same number of valence electrons.

What do transition metals have in common regarding their electron configurations?

All transition metals have partially filled d-orbitals.

What are the symbols for the 8 metalloids?

B, Si, Ge, As, Sb, Te, Po.

What group number do alkali metals belong to?

Group 1.

What group number do alkaline earth metals belong to?

Group 2.

What group number do halogens belong to?

Group 17.

What group number do noble gases belong to?

Group 18.

Which is the most electronegative? Pd, I, Cl, Cb

Cl

True or False: Na is larger than Na+. This is because Na has an additional energy level

true

Which of the following has the smallest atomic radius B, Ne, O, Li

Ne

true or false: F- is larger than F. This is because F- has an additional energy level

false

Which has the largest first ionization energy: O, Be, Li, Ne?

Ne

An anion will form from a when electrons are _

nonmetals;gained

Which noble hgas had the smallest atomic radius: Xe, Ne, Ar, Kr?

Ne

Which of the following is the most reactive (loses electrons more easily K, Na, Cs, Li

Cs

Which is the most electronegative: I, Rb, Cl, Sn?

Cl

What charge will aluminum acquire when it has a full outer energy level

3+

Which of the following has the largest radius: Li, Rb, Na, K

RB

Which of the following has the largest radius: Na+, F-, Ne, Mg2+

F-

Which of the following has the highest first ionization energy

Ca, Br, Sr, F

true or false: A metal generally will gain 1 or more electrons and acquire a positive charge

false

Which of the following is true regarding size? N3- > O2-, Ne>F-, Mg2+>Mg, F>F-

N3- > O2-

increases across a period, is a true trend for which two?

Ionization energy and electronegativity

True or False: Is a cation generally smaller than the neutral atom from which it is formed

true

What is the name of the Alkaline Earth metal in period 3?

Mg

Which of the following explains the group trend for Ionization energy

A.) Ionization energy decreases because the valence electrons are close to the nucleus

B.) Ionization energy increases because the valence electrons are closer to the nucleus

C.Ionization energy increases because the valence electrons are farther from the nucleus

D. ionization energy decreases because the valence electrons are a greater distance away from the nucleus

D

Which of the following has the largest radius: Sn, Te, S, Sb

Sn

Which of the following is the least reactive: Ne, Cu, F, Na

Ne

Which of the following explains the group trend for atomic radius?

A.) The size of atoms tends to increase down a group because additional shells are being added

B.) The size of atoms tends to increase down a group because electrons are added into the same energy

C.) The size of atoms tends to increase down a group because there is an increase in the number of valence electrons

D.) The size of atoms tends to increase down a group because shielding remains constant.

A

Which of the following explains the period trend for atomic radius?

A.) The size of atoms tends to decrease across a period because the number of shells increases, as well as the number of protons

B.)The size of atoms tends to decrease across a period because the number of valence electrons remains constant

C.)The size of atoms tends to decrease across a period because the valence electrons are higher energy levels

D.) The size of atoms tends to decrease across a period because the number of shells remains constant, and valence electrons are more strongly attracted to the nucleus

D