Chapter 14 Test

Question 1

What is the atomic radius?

Answer 1

half the distance between the nuclei of two alike atoms when bonded together in an atomic molecule.

Question 2

How are atomic radii trending in groups?

Answer 2

Increases as you move down a group

Question 3

Why do atomic radii increase as you go down a group?

Answer 3

There are more energy levels, which causes the atom to be larger.

Question 4

Describe the Shielding Effect with respect to atomic radius.

Answer 4

With each additional energy level, these inner energy levels block the pull of the nucleus on the outer electrons.

Question 5

What is the Shielding Effect?

Answer 5

When inner energy levels block the pull of the nucleus on the electrons of the outer energy levels.

Question 6

How does atomic radius trend in a period?

Answer 6

Decreases as you move to the right in a period.

Question 7

Why does atomic radius trend in a period?

Answer 7

There is increased nuclear charge as you move right in a particular period, without adding another energy level, so the electrons are pulled closer to the nucleus and atomic size decreases.

Question 8

Describe the Shielding Effect’s trends.

Answer 8

Increases going down a group, remains constant in the same period.

Question 9

What is Ionization energy?

Answer 9

The amount of energy needed to remove an electron from an atom

Question 10

What is the symnbol for ionization energy?

Answer 10

IE

Question 11

How does IE trend in a group?

Answer 11

As you go down a group, the energy decreases

Question 12

Why does IE trend the way it does in groups?

Answer 12

The larger the atom, the less energy needed to remove electrons from it because the nucleus has a weaker threshold on the outer electron shells.

Question 13

How does IE trend in a period?

Answer 13

As you go right in a period, this increases

Question 14

Why does IE trend the way it does in periods?

Answer 14

The nuclear charge increases, which decreases the size of the atom, as more eletrons are added. Becuase the electrons are held tighter together, it will take more energy to pull off those electrons because of the strong hold it has.

Question 15

Describe the relation between Shielding Effect and IE.

Answer 15

Because Shielding Effect increases, outer electrons aren’t held as tightly, so they are easier to remove and this requires less energy and a lower IE.

Question 16

Are noble gases part of the periodic trends? Explain.

Answer 16

No. They are completely stable, so they do not want to gain or lose any electrons. They are only counted for atomic radius because of their number of electrons.

Question 17

Which elements have the largest and smallest atomic radius?

Answer 17

Francium-largest

Helium-smallest

Question 18

Which elements have the highest and lowest IE?

Answer 18

Francium-lowest

Fluorine-highest

Question 19

Which elements have the highest and lowest electronegativity?

Answer 19

Francium-lowest

Fluorine-highest

Question 20

Why are the alkali metals so reactive?

Answer 20

They are the largest elements and have the lowest IE, so any electron can be removed at any time, which makes them quickly react.

Question 21

What is the first IEs?

Answer 21

The energy needed to remove the first electron from an atom.

Question 22

What is the second IE?

Answer 22

The energy needed to remove the second electron from an atom.

Question 23

When does a large jump occur in IE for an atom? Why does it do this?

Answer 23

When the atom attains noble gas electron configuration. It does this because it would take much more IE to remove one more atom from the noble gas configuration because it is most stable at a noble gas.

Question 24

What is the symbol for electronegativity?

Answer 24

EN

Question 25

What is electronegativity?

Answer 25

The tendency of an atom to attract electrons to itself when bonding to another atom.

Question 26

How does EN trend in groups?

Answer 26

It goes down as you move down a group.

Question 27

How does EN trend in periods?

Answer 27

It goes up as you move right in a period.

Question 28

Why does EN decrease during its trend in groups?

Answer 28

As you increase the number of energy levels and the Shielding Effect, atoms get larger, which means outer electrons are not held as tightly, so the atom has a lower ability to attract electrons to itself.

Question 29

Why does EN increase as you move across a period?

Answer 29

As nuclear charge increases across a period, atoms become smaller, thus holding their electrons closer and tighter, therefore having a greater ability to attract electrons, let alone hold on to their own.

Question 30

Which elements have highest and lowest EN?

Answer 30

Fluorine-highest

Francium-lowest

Question 31

How does Shielding Effect relate to energy levels?

Answer 31

If energy level size is larger, even though positive charges go up more by each period, the atom gets bigger because the spread of each energy level is larger.

Question 32

What is the ionic radius?

Answer 32

The size of an ion

Question 33

How does ionic radius trend in groups? Periods?

Answer 33

Increases down a group (same reasons as atomic radius)

Decreases across a period (same reasons as atomic radius)

Question 34

Why are cations always smaller than their neutral atoms?

Answer 34

Less electron repulsion is present because they lose electrons and are more positive.

Question 35

Why are anions always bigger than their neutral atoms?

Answer 35

More electron repulsion is present because they gain more electrons in bonding and are more negative.

Question 36

Why do metals form cations and nonmetals for anions?

Answer 36

They lose electrons to be noble, and they are easy to pull off electrons. Nonmetals are tighter, harder to pull apart because they have more electrons to start with and they have to gain to be noble.

Question 37

Describe EN, IE, AR, and IR with relation to metals and nonmetals.

Answer 37

Metals: low EN and IE
Nonmetals: high EN and IE