Chapter 2 - Periodic Table

Question 1

The first version of the periodic table of the elements was published by who? What did he order them with? And what are they now ordered by?

Answer 1

Dmitri Mendeleev, he ordered them according to atomic weight

Since then Henry Moseley revised it organizing elements based on increasing atomic number rather than atomic weight

Question 2

What does the periodic law say?

Answer 2

The chemical and physical properties of the elements are dependent, in a periodic way upon their atomic numbers

Question 3

The modern periodic table is arranged how? (Laterally and vertically)

Answer 3

With periods (rows), and groups or families (columns)

Question 4

There are 7 periods, what does this represent?

Answer 4

The principal quantum numbers n1-n7

Question 5

Groups contain elements that have similar…

Answer 5

Electronic configuration in their valence shell and share similar chemical properties

Question 6

What does the Roman numeral above each group represent?

Answer 6

The number of valence electrons that the element has in that group when in a neutral state

Question 7

Letters A and B separates the elements into 2 larger groups, what else is A and B elements called?

Answer 7

A elements are known as representative elements

B elements are known as nonrepresentative elements

Question 8

What groups are in the A elements? What are their subshells?

Answer 8

Includes groups IA-VIIIA, have either S or P subshells

Question 9

What groups of elements are in B elements? What are their subshells?

Answer 9

Include both the transitional elements (subshells s, and d), and the actinide and lanthanide series (subshells s, and f)

Question 10

For A and B elements what does it tell you about their electron configuration?

Answer 10

For A (representative elements) the Roman numeral and the letter designation determine the electron configuration

For B (nonrepresentative elements) they may have unexpected electron configuration

Question 11

What 3 groups of elements can the periodic table be divided into with similar characteristics?

Answer 11

Metals, nonmetals, metalloids (semimetals)

Question 12

Where are metals found on the periodic table and what series’s do they include?

Answer 12

Left side and middle of periodic table

Include active metals, transition metals, actinide, and lanthanide series

Question 13

Metals are generally what?

Answer 13

Lustrous (shiny) solids, have high melting points, and density

Question 14

Metals have the ability to…

Answer 14

Be deformed without breaking

Be hammered into shapes (called malleability)

Be pulled or drawn into wires (called ductility)

Question 15

At an atomic level metal is defined by…

Answer 15

A low effective nuclear charge, low electronegativity (high electropositivity), large atomic radius, small ionic radius, low ionization energy, and low electron affinity (easily give up electrons)

Question 16

Many of the transition metals have 2 or more oxidative states meaning

Answer 16

Charges when forming bonds with other atoms

Question 17

Why are metals good conductors of heat and electricity

Answer 17

Because valence electrons of metals are loosely held to their atoms, letting them move freely

Question 18

Active metals are found in what subshells?

Answer 18

S subshells

Question 19

Where are nonmetals found on the periodic table?

Answer 19

Upper right side

Question 20

List as many characteristics of nonmetals as you can

Answer 20

-Generally brittle in the solid state

-Show little or no metallic luster

-Have high ionization energies, electron affinities, and electronegativity

-small atomic radii and large ionic radii

-usually poor conductors of heat and electricity

-Inability to easily give up electrons

-less unified in their chemical and physical properties than the metals

Question 21

What seperates metals and non metals?

Answer 21

Metalloids

Question 22

Name all the nonmetals and what is the group known as

Answer 22

Known as a stair step group of elements

Includes: Boron (B), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te), polonium (Po), and astatine (At)

Question 23

Characteristics of metalloids

Answer 23

-Electronegativities and ionization energies of the metalloids lie between those of metals and non metals

-Physical properties, densities, boiling points, melting points vary widely

-Reactivities of the metalloids are dependent on the elements with which they are reacting (can act as metal or nonmetal)

Question 24

The electrostatic attraction between the valence shell electrons and the nucleus is know as…

Answer 24

The effective nuclear charge (Zeff) - a measure of the net positive charge experienced by the outermost electrons

Question 25

On the periodic table how does Zeff increase?

Answer 25

It increases up and to the right

Question 26

What group are the noble (inert) gases

Answer 26

Group 18

Question 27

When do elements tend to be most stable?

Answer 27

When valence shell is full

Question 28

On the periodic table where does atomic radius increase?

Answer 28

Going down and to the left

Question 29

Out of metals and non metals which ones tend to gain or lose electrons?

Answer 29

Metals lose electrons and become positive while nonmetals gain electrons and become negative

Question 30

Metalloids can go either way but tend to follow the trend based on what?

Answer 30

Which side of the metalloids line they fall on

Question 31

Do nonmetals closer to the metalloid line poses a larger or smaller ionic radius than their counterparts closer to group 18?

Answer 31

Larger

Question 32

Is the ionic radius of metals near the metalloids line smaller or larger than other metals?

Answer 32

Smaller

Question 33

Ionization energy is also known as

Answer 33

Ionization potential

Question 34

What is ionization energy?

Answer 34

The energy required to removed an electron from a gaseous species

Question 35

Removing an electron from an atom always required a input of heat, making it what type of process?

Answer 35

Endothermic process

Question 36

The greater the Zeff of an atom correlates how to ionization energy?

Answer 36

The greater the Zeff the more tightly bound they are, making it more difficult to remove one or more electrons, this increases the ionization energy

Question 37

On the periodic table where does ionization energy increase?

Answer 37

Up and to the right

Question 38

Energy necessary to remove the first electron and second electron are called what?

Answer 38

The first and second ionization energy

Question 39

What group is least likely to give up an electron

Answer 39

The noble or inert gases (group 18)

Question 40

What group is the most greedy group for electrons?

Answer 40

The halogens (group 17)

Question 41

What process expels energy in the form of heat

Answer 41

Exothermic processes

Question 42

What is electron affinity?

Answer 42

The energy dissipated by a gaseous species when it gains an electron - opposite concept of ionization energy

Question 43

Exothermic processes have a negative sign but the electron affinity is reported as a positive number, why is this?

Answer 43

Because it is the sum of dissipated energy

Question 44

The higher electrostatic pull is equal to

Answer 44

Higher Zeff or effective nuclear charge

Question 45

The stronger the electrostatic pull between the nucleus and the valence shell equals greater energy release when the atoms gain an electron. Why is this?

Answer 45

This is because the electron has to overcome a stronger attraction from the nucleus to be added to the atom's electron cloud.

Question 46

Where on the periodic table does electron affinity increase?

Answer 46

Up and to the right

Question 47

Those with lower electron affinities are less likely to what?

Answer 47

Gain an electron

Question 48

What group has the lowest electron affinity?

Answer 48

The noble gases. This is because they have full electron shells and are highly stable, so they are generally not inclined to gain or lose electrons.

Question 49

What is electronegativity?

Answer 49

The measure of the attractive forces that an atom will exert on an electron in a chemical bond The greater the electronegativity of an atom the greater it attracts electrons within a bond

Question 50

What is the main exception to the electronegativity trend on the periodic table?

Answer 50

The noble gases, specifically the first 3 because they do not often form bonds

Question 51

What does the Pauling electronegativity scale range from on elements? (Highest and lowest)

Answer 51

.7 for Cesium (least electronegative) to 4.0 for fluorine (most electronegative)

Question 52

What is the trend for increasing electronegativity on the periodic table?

Answer 52

Up and to the right

Question 53

What are the trends for the periodic table for electronegativity, atomic radius, ionization energy, and electron affinity

Answer 53

Electronegativity, ionization energy, and electron affinity increase up and to the right on the periodic table Atomic radius increases down and to the left on the periodic table

Question 54

What is the name of group 1 on the periodic table?

Answer 54

Alkali metals

Question 55

List some characteristics of alkali metals?

Answer 55

-Densities are lower than those of other metals -Have one loosely bound electron in their outermost shells -React readily with nonmetals-especially halogens

Question 56

What is the name of group 2 on periodic table?

Answer 56

Alkaline Earth metals

Question 57

Together group 1 and group 2 on the periodic table are called…

Answer 57

Active metals because they are so reactive that they are not naturally found in their elemental (neutral) state

Question 58

Characteristics of alkaline earth metals valence electrons?

Answer 58

They have 2 electrons in their valence shell, both of which are easily removed to form divalent cations

Question 59

Group 16 on the periodic table is called what?

Answer 59

The Chalcogens

Question 60

Even though Chalcogens are very biologically useful, at high concentrations they can be…

Answer 60

Toxic or damaging

Question 61

What is the name of group 17 on the periodic table?

Answer 61

The Halogens

Question 62

Characteristics of Halogens

Answer 62

Highly reactive nonmetals Desperate to complete their octet by gaining one additional electron Are so reactive that they are not naturally found in their elemental state but rather as ions called halides

Question 63

What element has the highest electronegativity?

Answer 63

Fluorine (F)

Question 64

What are noble gases also called?

Answer 64

Inert gases

Question 65

Why do noble gases have minimal chemical reactivity?

Answer 65

Because of their filled valence shells

Question 66

Noble gasses characteristics

Answer 66

Extremely low boiling points Exist as gases at room temperature

Question 67

Why are transition metals good conductors?

Answer 67

Due to their loosely held electrons that progressively fill their d-orbitals in their valence shell

Question 68

Many of the transition metals can have different possible charged forms or oxidation states because of what?

Answer 68

Their capability of losing different numbers of electrons from the s and d orbitals in their valence shell - this forms many different ionic compounds

Question 69

For transition metals formation of complexes causes the d-orbitals to split into energy sub levels, enabling…

Answer 69

Many of the complexes to absorb certain frequencies of light, frequencies not absorbed give the complexes their characteristic colors, giving way to electron transitions

Question 70

When we perceive an object as a particular color, it is because that color is not absorbed but rather…

Answer 70

Is the color Reflected by the object

Question 71

If an object absorbs a given color of light and reflects all others how does our brain arrive at a perception of color?

Answer 71

Our brain mixes these subtraction frequencies and we perceive the complementary color of the frequency that was absorbed

Question 72

What groups on the periodic table are most reactive with water

Answer 72

Groups 1 and 2

Question 73

What groups have 6 valence electrons

Answer 73

6, and 16

Question 74

What groups contain atleast 1 metal?

Answer 74

Groups 1-15

Question 75

All groups contain multiple oxidative states but most notably what groups do?

Answer 75

3-12 (transition metals)

Question 76

All groups have negative oxidative states but most notably…

Answer 76

Groups 14-17