Chapter 5- The Periodic Law

Question 1

What is the principal energy level?

Answer 1

The major energy level of electrons

Indicated by the principal quantum number

Question 2

What is the principal quantum number?

Answer 2

(n) Indicates the relative size and shape of orbitals.

Question 3

If its principal energy level 1, it has ____ sublevels

Answer 3

1

Question 4

What is the shape and # of orbitals for the s orbital?

Answer 4

Spherical

1

Question 5

What is the shape and # of orbitals for the p orbital?

Answer 5

Bowtie

3

Question 6

What is the shape and # of orbitals for the d orbital?

Answer 6

Multiple

5

Question 7

What is the shape and # of orbitals for the f orbital?

Answer 7

Multiple

7

Question 8

What is electron configuration?

Answer 8

The arrangement of electrons in an atom.

Question 9

On the periodic table, groups go…

Answer 9

Left to right

Question 10

On the periodic table, periods go…

Answer 10

Up and down

Question 11

What are valence electrons?

Answer 11

Outermost electrons in an atom.

Question 12

Elements in a _____ have the same number of valence electrons

Answer 12

Group

Question 13

Elements in a ____ have the same principle energy level.

Answer 13

Period

Question 14

What did Mendeleev do to create the first periodic table

Answer 14

He showed a connection between atomic mass and elemental properties and arranged electrons with similar properties into columns

Question 15

What did Moseley do to fix Mendeleev’s table?

Answer 15

He discovered that each element had a unique atomic number and arranged the elements in the table according to their increasing atomic number

Question 16

What is the periodic law?

Answer 16

When arranged by increasing atomic number, the elements exhibit a periodic repetition of chemical and physical properties.

Question 17

Where are metalloids on the periodic table?

Answer 17

The staircase

Question 18

What orbital block are transition metals?

Answer 18

d

Question 19

What orbital block are inner transition metals?

Answer 19

f

Question 20

Describe metals in terms of appearance, state at room T, and conductivity

Answer 20

Shiny/luster when smooth and clean, solid at room T, good conductors

Question 21

Describe nonmetals in terms of appearance, state at room T, and conductivity

Answer 21

Tend to be gases but dull and brittle solids, poor conductors

Question 22

What group and reactivity are alkali metals?

Answer 22

Group 1

Highly reactive

Question 23

What group and reactivity are alkaline earth metals?

Answer 23

Group 2

Highly reactive

Question 24

Whats another name for inner transition metals?

Answer 24

Lanthanide and Actinide Series

Question 25

What group and reactivity are halogens?

Answer 25

Group 17

Highly reactive

Question 26

What group and reactivity are the noble gases?

Answer 26

Group 18

Virtually unreactive

Question 27

For atomic radius, whats the trend across the periods and groups?

Answer 27

Periods- increase

Groups- decrease

Question 28

For ionization energy, whats the trend across the periods and groups?

Answer 28

Periods- decrease

Groups- increase

Question 29

For electronegativity, whats the trend across the periods and groups?

Answer 29

Periods- decrease

Groups- increase

Question 30

What is ionization energy

Answer 30

The energy required to remove one electron from a neutral atom of an element

Question 31

What is electronegativity?

Answer 31

A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound