[CHEM] Unit 6- The Periodic Table

Question 1

The periodic table is arranged by increasing ___

Answer 1

Atomic number

Question 2

Having luster, being hard and malleable, and becoming cations are characteristics of ___

Answer 2

Metals

Question 3

T/F: All metals are liquid, except for Hg

Answer 3

F- all metals are solid, except for Hg

Question 4

T/F: Metals are conductors of heat and electricity

Answer 4

T

Question 5

Being very brittle and anions are characteristics of ___

Answer 5

Nonmetals

Question 6

T/F: Nonmetals CANNOT exist in all three states of matter

Answer 6

F- Nonmetal elements can exist in all three states of matter

Question 7

T/F: Nonmetals cannot conduct electricity

Answer 7

T

Question 8

The following elements are metalloids: ___

Answer 8

B, Si, As, Te, At, Ge, and Sb

Question 9

The exceptions of metalloids are ___

Answer 9

Al and Po

Question 10

T/F: Metalloids have a mix of metal and nonmetal characteristics

Answer 10

T

Question 11

Only ___ and ___ are liquids at STP

Answer 11

Hg, Br

Question 12

Other than noble gases, the following elements are gases:

Answer 12

H,N,O,F,Cl

Question 13

Melting and boiling points tend to ___ going ___ a group

Answer 13

Increase, down

Question 14

A row or ___ is ____

Answer 14

Period, horizontal

Question 15

A group, ___, or ___ are ___

Answer 15

Family, column, vertical

Question 16

Elements in the same period have the same ___

Answer 16

Number of occupied shells/PELs

Question 17

T/F: Hydrogen is in its own group

Answer 17

T- hydrogen is the only nonmetal on the left and can be -1 or +1

Question 18

Group 1 are ___

Answer 18

Alkali metals

Question 19

Characteristics of alkali metals include:

Answer 19

Being the most reactive (react with water), not isolated in nature, ignites when reacted, and +1 charge

Question 20

Alkali metals are ___ reactive going ___ the group

Answer 20

More, down

Question 21

Group 2 are ___

Answer 21

Alkaline earth metals

Question 22

Characteristics of alkaline earth metals include:

Answer 22

Being reactive, not isolated in nature, and +2 charge

Question 23

Groups 3-11 are ___

Answer 23

Transition metals

Question 24

Characteristics of transition metals include:

Answer 24

Multiple oxidation states (due to D sublevels being filled), producing colored solutions when dissolved, and typical metal properties

Question 25

All elements that are Z<___, or have more than ___ electrons/protons are ___

Answer 25

83, radioactive

Question 26

The detached rows of the table are ___

Answer 26

Inner transition metals

Question 27

The top row of the inner transition metals start with ___ and is called the ___

Answer 27

Lanthanum, Lanthanide series

Question 28

The bottom row of the inner transition metals start with ___ and is called the ___

Answer 28

Actinium, Actinide series

Question 29

T/F: ALL of the Actinide series are radioactive

Answer 29

T- they are also called Rare Earth Metals

Question 30

Groups 12-16 are called ____

Answer 30

They do not have names

Question 31

Group 17 are ___

Answer 31

Halogens

Question 32

Characteristics of halogens include:

Answer 32

-1 charge, being the most reactive nonmetals, all 3 states of matter, are not isolated in nature

Question 33

In the halogens, the boiling point goes ___ going ___

Answer 33

Up, down

Question 34

Group 18 are ___

Answer 34

Noble gases

Question 35

Characteristics of noble gases include:

Answer 35

Full valence shell (not reactive), monatomic, all are gases

Question 36

Only ___ noble gases bond with F because of its high ___

Answer 36

Large, electronegativity

Question 37

Metallic characteristics increase going ____

Answer 37

Down

Question 38

Reactivity for nonmetals ___ going left-right and ___ going top-bottom because of electron ___

Answer 38

Increases, decreases, affinity

Question 39

Reactivity for metals increases ___ and decreases ___ due to ___

Answer 39

Top to bottom, left to right, ionization energy

Question 40

Atomic radius is ___

Answer 40

The measurement of 1/2 the distance between nuclei when bonded

Question 41

Atomic radius ___ going ___ a group because of more PELs

Answer 41

Increases, down

Question 42

Atomic radius ___ going left-right because of ___

Answer 42

Decreases, more protons (greater nuclear charge)

Question 43

T/F: Halogens are larger than noble gases

Answer 43

F- the exception to atomic radius; noble gases are actually larger

Question 44

When metals form ___, they become ___

Answer 44

Cations, smaller

Question 45

When nonmetals form ___, they become ___

Answer 45

Anions, larger

Question 46

ELectronegativity is defined as ___

Answer 46

An atom’s attraction to electrons IN A BOND

Question 47

Electronegativity is higher for ___

Answer 47

Nonmetals

Question 48

Electronegativity ___ going left-right because ___

Answer 48

Increases, greater nuclear charge

Question 49

Electronegativity ___ going top-bottom because ___

Answer 49

Decreases, increased shielding and larger distance to nucleus

Question 50

Electron affinity is defined as ___

Answer 50

The energy released when an electron is added, or the likelihood of an atom gaining an electron

Question 51

Electron affinity ___ going top-bottom due to ___

Answer 51

Decreases, shielding

Question 52

“Shielding” is ___

Answer 52

When inner electrons block outer electrons

Question 53

Electron affinity ___ going left-right because of ___

Answer 53

Increases, more protons

Question 54

Na+1 is smaller than Mg+2 because of ___ radii due to ___ protons

Answer 54

Smaller, more

Question 55

Ionization energy is ___

Answer 55

The energy required to completely remove a valence electron

Question 56

Ionization energy ___ going left-right due to greater ___ and ___ going down due to ___ (hint: less pull on electrons!)

Answer 56

Increases, greater nuclear charge (more pull from protons), decreases, shielding

Question 57

To determine how many valence electrons an atom has, you must ___

Answer 57

Compare the values- where the biggest jump is, the last ve is