Periodic Properties

Question 1

Periodic Law

Answer 1

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

Question 2

Periods

Answer 2

the rows on the periodic table

Question 3

Groups

Answer 3

• The columns on the periodic table
• represent elements that have the same electronic configuration in their valence shell and share similar chemical properties

Question 4

Representative elements

Answer 4

• have either s o p sublevels as their outermost orbitals

- Groups IA through VIIA, all of which have incompletely filled s or p subshells of the highest principal number

Question 5

Nonrepresenatative elements

Answer 5

-include transition elements, which have partially filled d sublevels

Question 6

Atomic Radius

Answer 6

equal to one-half the distance between the centers of two atoms of that element that are just barely touching each other

Question 7

Ionic Radius

Answer 7

the radius of a cation or an anion

Question 8

Ionization Energy (IE)

Answer 8

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

Question 9

First ionization energy

Answer 9

the energy required to remove on valence electron from the parent atom

Question 10

Second Ionization Energy

Answer 10

the energy needed to remove a second valence electron from the univalent ion to form the divalent ion

Question 11

Electron Affinity (EA)

Answer 11

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 electorn

Question 12

Alkaline Earth Metals

Answer 12

have low electron affinity values, these elements are relatively stable because their s subshell is filled

Question 13

Halogens

Answer 13

have high electron affinities because the addition of an electron to the aotm results in a completely filled shell, which represents a stable electron configuration

Question 14

Electronegativity

Answer 14

a measure of the attraction an atom has for electrons in a chemial bond.

Question 15

Pauling electronegativity scale

Answer 15

the values range from 0.7 (the most electropositive) for the most electropositive elements to 4.0 (the most electronegative)

Question 16

Metals

Answer 16

• found on the left side of the periodic table
• shiny solids at room temperature and generally have high melting points and densities
• have the ability to be deformed without breaking
• have large atomic radius, low ionization energy, and low electronegativity
• few electrons in the valence shell of a metal atom can easily be removed
• good conductors of heat and electricity

Question 17

Malleability

Answer 17

the ability of a metal to be hammered into shapes

Question 18

Ductility

Answer 18

the ability of metals to be drawn into wires

Question 19

Nonmetals

Answer 19

• generally brittle in the solid state and show little or no metallic luster
• have high ionization energies and electronegativities and are usually poor conductors of heat and electricity
• has the ability to gain electrons easily
• located on the upper right side of the periodic table and are separated from the metals by a line cuttting diagonally through the region of the periodic table containing elements with partially filled p orbitals

Question 20

Metalloids

Answer 20

• found along the line between the metals and nonmetals in the periodic table and their properties vary considerably
• densities, boiling points, and melting points fluctuate widely
• the electronegativies and ionization energies of metalloids lie between those of metals and nonmetals
• the reactivity is dependent upon the element with which they are reacting

Question 21

Ions

Answer 21

-ionic compounds are made up of cations and anions, where a cation is a positive ion and an anion is a negative ion

Question 22

Hydrogen

Answer 22

• has a large single s valence electron and forms the H+ ion
• it can also form the hydride ion H-
• resembles the halogens in that it only requires on additional electron to reach the next noble gas configuration

Question 23

Alkali Metals

Answer 23

• the elements of Group IA
• possess most of the physical properties common to metals, yet their densities are lower than those of other metals
• have only one loosely bound electron in their outermost shell, giving them the largest atomic radii of all elements in their respective periods
• they can lose their valence electron to form univalent cations, allowing them to easily form +1cations

Question 24

Alkali Earth Metals

Answer 24

-the elements of Group IIA
-dependent on the ease with which they lose
electrons
-have two electrons in their outer shell and have smaller atomic radii than the alkali metals, which can be removed to form divalent cations
-commonly form +2cations

Question 25

Carbon Group

Answer 25

• the family containing carbon, group IVA
• have two electrons in their outermost p subshells
• tends not to form ions, but participates in electron sharing (four covalent bonds)

Question 26

Pnictogens

Answer 26

• nitrogen and the elements below it in group VA
• forms covalent bonds but most commonly forms three per atom
• commonly holds a positive charge in organic reactions (a good base)

Question 27

Chalcogens

Answer 27

• group VIA
• elements requiring two additional valence electrons to complete their outermost shells
• tend to be fairly electronegative and to form -2 anions, but can also participate in covalent bonds

Question 28

Noble Gases

Answer 28

• also called inert gases, found in Group VIIIA
• completely nonreactive b/c they have complete valence shells
• no tendency to gain or lose electrons, high ionization energies, and no electronegativities
• posses low boiling points and are gases at room temp