Chemistry - Periodic Table

Front 1

What does periodic law state?

Back 1

It says that the chemical properties of the elements are dependent, in a systematic way, upon their atomic numbers

Front 2

How are elements arranged?

Back 2

They are arranged in periods (rows) and groups (columns)

Front 3

How many periods are there?

Back 3

There are seven periods

Front 4

What do they represent?

Back 4

They represent the principal quantum numbers n = 1 to n = 7

Front 5

What do groups represent?

Back 5

They represent elements that have the same electronic configuration in their valence, or outermost shell

Front 6

What do things in the same group share?

Back 6

They share similar chemical properties

Front 7

What are the electrons in the outermost shell called?

Back 7

They are called valence electrons

Front 8

What are the A elements called?

Back 8

They are called the representative elements

Front 9

What do the A elements have as their outermost orbitals?

Back 9

They have either s or p sublevels

Front 10

What are the B elements called?

Back 10

They are the nonrepresentative elements

Front 11

What partly filled sublevels do the transitions elements have?

Back 11

They have partly filled d sublevels

Front 12

What partly filled sublevels do the lanthanide and actinide series have?

Back 12

They have partially filled f sublevels

Front 13

What is the ionization potential?

Back 13

It is the energy required to completely remove an electron from a gaseous atom or ion

Front 14

What does removing an electron from an atom always require?

Back 14

It always requires an input of energy

Front 15

How does ionization energy relate to the distance from an electron to its nucleus?

Back 15

The closer and more tightly bound an electron is to the nucleus, the more difficult it will be to remove

Front 16

What is the first ionization energy?

Back 16

It is the energy required to remove one valence electron from the parent atom

Front 17

What is the second ionization energy?

Back 17

It is the energy needed to remove a second valence electron from the univalent ion to form the divalent ion, and so on

Front 18

Which ionization energy is more, the first or second energy?

Back 18

The second ionization energy is always greater than the first

Front 19

What is electron affinity?

Back 19

It is the energy change that occurs when an electron is added to a gaseous atom, and it represents the ease with which the atom can accept an electron

Front 20

How does attractive pull relate to electron affinity?

Back 20

The strong the attractive pull of the nucleus for electrons, the greater the electron affinity will be

Front 21

What electron affinities do the noble gases have?

Back 21

They have electron affinities on the order of zero, since they already possess a stable octet and cannot readily accept an electron

Front 22

What is electronegativity?

Back 22

It is the measure of the attraction an atom has for electrons in a chemical bond

Front 23

What characteristics do metals have?

Back 23

They are shiny solids except for mercury at room temperature, and they have high melting points and densities

Front 24

What is malleability?

Back 24

It is the ability of a metal to be hammered into shapes

Front 25

What is ductility?

Back 25

It is the ability of a metal to be drawn into wires

Front 26

What are some other characteristic properties?

Back 26

They have a large atomic radius, low ionization energy, and low electronegativity

Front 27

What are those factors due to?

Back 27

They are due to the fact that the few electrons in the valence shell of a metal atom can easily be removed

Front 28

What does this imply about their conductivity?

Back 28

Because the valence electrons can move freely, metals are good conductors of heat and electricity

Front 29

What are the most reactive metals?

Back 29

Group IA and IIA are the most reactive metals

Front 30

What are characteristics of nonmetals?

Back 30

They are generally brittle in the solid state and show little or no metallic luster

Front 31

What about their ionization energies?

Back 31

They have high ionization energies and electronegativities

Front 32

Do the conduct?

Back 32

They are usually poor conductors of heat and electricity

Front 33

Do nonmetals gain electrons easily?

Back 33

Most nonmetals share the ability to gain electrons easily

Front 34

What are alkali metals?

Back 34

They are the elements of Group IA

Front 35

What are their densities?

Back 35

Their densities are lower than those of other metals

Front 36

How are their atomic radii?

Back 36

They have only one loosely bound electron in their outermost shell

Front 37

Do they readily lose or gain electrons?

Back 37

They readily lose their valence electron to form univalent cations

Front 38

What are alkaline earths?

Back 38

They are the elements of Group IIA

Front 39

How are their atomic radii?

Back 39

They have smaller atomic radii than the alkali metal

Front 40

Do they gain or lose electrons?

Back 40

They have two valence electrons that are not held very tightly to the nucleus, so they can be removed to form divalent cations

Front 41

What are halogens?

Back 41

They are Group VIIA. They are highly reactive nonmetals with seven valence electrons

Front 42

What are noble gases?

Back 42

They are also called inert gases, and they are found in Group VIII

Front 43

Are they reactive?

Back 43

They are fairly nonreactive because they have a complete valence shell

Front 44

Do they have high or low boiling points?

Back 44

They have low boiling points?

Front 45

Are the transition elements metals?

Back 45

They are all considered metals

Front 46

Do they have high or low melting and boiling points?

Back 46

They have high melting and boiling points