chemistry chapter 2

Question 1

periodic law

Answer 1

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

Question 2

periods

Answer 2

rows. 7 of them, representing the principal quantum numbers n=1 to n=7, and each period is filled sequentially

Question 3

groups

Answer 3

columns. Represent elements that have the same electronic configuration in their valence, or outermost shell, and share similar chemical properties

Question 4

valence electrons

Answer 4

electrons in the outermost shell. Involved in chemical bonding and determine the chemical reactivity and properties of the element

Question 5

representative elements

Answer 5

which have either s or p sublevels as their outermost orbitals. A elements

Question 6

nonrepresentative elements

Answer 6

including transition elements, which have partially filled d sublevels, and the lanthanide and actinide series, which have partly filled f sublevels. B elements

Question 7

atomic radius

Answer 7

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

Question 8

ionization energy (IE)

Answer 8

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

Question 9

first ionization energy

Answer 9

is the energy required to remove one valenece electron from the parent atom

Question 10

second ioniztion energy

Answer 10

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

Question 11

electron affinity

Answer 11

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

Question 12

group IIA elements

Answer 12

alkaline earths, have low electron affinity values. Are relatively stable because their s subshell is filled

Question 13

group VII elements

Answer 13

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

Question 14

group VIII elements

Answer 14

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

Question 15

electronegativity

Answer 15

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

Question 16

metals

Answer 16

are shiny solids at room temperature, and generally have high melting points and densities

Question 17

malleability

Answer 17

the ability of metal to be hammered into shapes

Question 18

ductility

Answer 18

ability to be drawn into wires

Question 19

nonmetals

Answer 19

are generally brittle in the solid state and show little or no metallic luster. They have high ionization energies and electronegativities, and are usually poor conductors of heat and electricity

Question 20

metalloids

Answer 20

their densities, boiling points, and melting points fluctuate widely. Elements classified as metalloids are boron, silicon, germanium, arsenic, antimony, and tellurium

Question 21

alkali metals

Answer 21

are the elements of group IA. They posses 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 the elements in their respective periods

Question 22

alkaline earths

Answer 22

are the elements of group IIA, which also possess many characteristically metallic properties. Have low electronegativities and positive electron affinities

Question 23

halogens

Answer 23

group VIIA, are highly reactive nonmetals with seven valence electrons (one short of the favored octet configuration. The electronegativities are very high, and they are particularly reactive towards alkali metals and alkaline earths, which “want” to donate electrons to the halogens to form stable ionic crystals

Question 24

noble gases

Answer 24

are found in group VIII. Are fairly nonreactive because they have a complete valence shell, which is an energetically favored arrangement. Gives them little to no tendency to gain or lose electrons, high ionization energies, and no real electronegativites. they possess low boiling points and are all gases at room temperature

Question 25

transition elements

Answer 25

groups IB to VIIIB, are all considered metals. Are very hard and have high melting oints and boiling points