Chapter 9: Electrons in Atoms and the Periodic Table

Question 1

Explain Wavelength

Answer 1

the distance between two consecutive waves

Question 2

Explain Frequency

Answer 2

how close or far the waves are

Question 3

Describe the relationship between wavelength and frequency

Answer 3

These two measurements are inversely related because

Question 4

Which has more energy, short or long wavelengths?

Answer 4

shorter wavelengths have more energy

Question 5

A specific color of light has a specific amount of energy measured by its wavelength. The color red has a longer wavelength than the color violet. Which color has the higher amount of energy?

Answer 5

Violet light has higher energy than red light.

Question 6

Describe the Bohr electron-energy-level-model of the hydrogen atom

Answer 6

Hydrogen atoms was exposed to electricity and produced light. The amount of energy released, and atoms absorbed determine the color of light. Concluded that electrons are located at different energy levels with different levels surrounding the nucleus

Question 7

electrons are described as both particles and energy waves

Question 8

electrons occupy different principal energy levels numbered 1, 2, 3, 4, 5, 6 and 7 which are progressively farther from the nucleus

Answer 8

Subshells

Question 9

within an energy level (or shell) there are one or more sublevels (or subshells) the electrons may occupy

Question 10

each sublevel (or subshell) contains one or more orbitals

Question 11

each orbital can hold up to two electrons

Question 12

electrons are always in motion

Question 13

all an atom’s electrons are visualized as a cloud surrounding the nucleus

Question 14

Define valence electrons.

Answer 14

The outermost electrons

Question 15

In what energy level are an atom’s valence electrons located?

Answer 15

The highest energy level

Question 16

Define core electrons.

Answer 16

electrons not in the outermost shell

Question 17

Remember that the representative elements in the same column have the same valence electron configuration.

Answer 17

2 right and 2 left columns

Question 18

Remember the locations of these families: alkali metals, alkaline earth metals, halogens and noble gases.

Answer 18

Alkali metals: first column. Alkaline earth metals: second column. Halogens: 17th (second to last) column. Noble gases: 18th (last) column

Question 19

Define atomic radius

Answer 19

Distance from the nucleus to the outermost (valence) electrons.

Question 20

List atomic radius periodic trend for a row in the periodic table of the elements.

Answer 20

Atomic radius increases going down the rows on the periodic table

Question 21

Explain the reason for the atomic radius periodic trend for a row.

Answer 21

The atomic radius gets smaller because the more protons the more the nucleus is brought them closer to it.

Question 22

List atomic radius periodic trend for a column in the periodic table of the elements.

Answer 22

Atomic radius increases going down a column in the periodic table

Question 23

Explain the reason for the atomic radius periodic trend for a column.

Answer 23

going down a column in the periodic table elements have more electrons. the more electrons the more shells that are occupied the bigger the atom

Question 24

Define ionization energy.

Answer 24

amount of energy needed to remove one valence electron from an atom in its gaseous state

Question 25

List the ionization energy periodic trend for a row in the periodic table of the elements.

Answer 25

Ionization energy increases from left to right

Question 26

Explain the reason for the ionization energy periodic trend for a row.

Answer 26

The smaller the radius of an atom the more Ionization energy is needed

Question 27

List ionization energy periodic trend for a column in the periodic table of the elements.

Answer 27

Ionization energy decreases from top to bottom

Question 28

Explain the reason for the ionization energy periodic trend for a column.

Answer 28

the bigger the radius the less ionization energy needed.

Question 29

Remember metals tend to lose electrons in chemical reactions while nonmetals tend to gain electrons.

Question 30

Describe the periodic trend for metallic character

Answer 30

move down diagonally

Question 31

Describe the periodic trend for nonmetallic character.

Answer 31

moving up diagonally