The Periodic Table

Question 1

What are the rows called?

Answer 1

periods

Question 2

What are the columns called?

Answer 2

groups

Question 3

What are A elements and where are the valence e-?

Answer 3

aka “representative elements” and include groups IA thorough VIIIA, valence electrons in the s or p subshells

Question 4

What are B elements and where are the valence e-?

Answer 4

aka “nonrepresentative elements”, include transition elements (valence e- in the s and d subshells), lanthanide and actinide series (valence e- in s and f subshells)

Question 5

Metals

Answer 5

lustrous (shiny) solids, generally high melting points, can be deformed without breaking (malleability/ductility), low electronegativity, large atomic radius, small ionic radius, low ionization energy, and low electron affinity. Found on the left side of the periodic table.

Question 6

What are oxidation states?

Answer 6

charges when forming bonds with other atoms or “different possible charged forms” ex: Cu+2

Question 7

What makes something a good conductor?

Answer 7

When the valence electrons are only help loosely so they are free to move around

Question 8

Nonmetals

Answer 8

brittle in solid state, no/little luster, high ionization energies, electron affinities, electronegativities, small atomic radii and large ionic radii, poor conductors in heat, inability to easily give up electrons, less unified in their chemical and physical properties, found in the upper right side of the periodic table

Question 9

Metalloids

Answer 9

aka “semimetals”, physical properties vary widely, combinations of nonmetals and metals, found in stair step group of elements

Question 10

Effective Nuclear Charge (Zeff)

Answer 10

a measure of the net positive charge experienced by the outermost electrons, attraction between the valence shell electrons and the nucleus, increases right to left across table, constant down groups

Question 11

What is the electrostatic trend?

Answer 11

as you move down a group, electrostatic attraction decreases

Question 12

Octet rule

Answer 12

elements gain or lose electrons to try and achieve a stable octet of valence electrons; many exceptions

Question 13

Atomic radius

Answer 13

is equal to one-half of the distance between the centers of two atoms of an element that are briefly in contact with each other, decreases right to left across table, increases down groups

Question 14

Ionic radii

Answer 14

In order to understand know that:
(1) metals lose electrons and become positive, while nonmetals gain electrons and become negative 
(2) metalloids can go either direction 
Metals - smaller ionic radius
Nonmetals - larger ionic radius

Question 15

Ionization energy (IE)/ ionization potential

Answer 15

energy required to remove an electron from a gaseous species, increases left to right and bottom to top

Question 16

Endothermic process

Answer 16

removing an electron which requires INPUT of heat

Question 17

Exothermic process

Answer 17

requires an electron which OUTPUTs energy as heat

Question 18

Relationship between Zeff and ionization energy

Answer 18

the higher the atoms Zeff, the higher the ionization energy. this is because Zeff is a measure of how close the valence electrons are being held to the nucleus (higher = closer) and so this makes it hard to remove requiring more energy (higher ionization energy)

Question 19

What is first ionization energy?

Answer 19

the energy required to remove the first electron

Question 20

Active metals

Answer 20

have extremely low ionization energies so much that they are almost always found naturally in ionic compounds instead of neutral forms, ex: Li and Be

Question 21

Electron affinity

Answer 21

basically how likely an element is to attract electrons to complete it’s octet but the actual definition is the energy dissipated by a gaseous species when it gains an electron, decreases top to bottom, increase left to right, “opposite of ionization energy”

Question 22

Relationship between Zeff and electron affinity

Answer 22

as Zeff increases, so does electron affinity. This is because the stronger the electrostatic pull the greater the energy release when an atom gains an electron

Question 23

Electronegativity

Answer 23

measure of the attractive force that an atom with exert on an electron in a chemical bond

Question 24

Relationship between electronegativity and ionization energy

Answer 24

the lower the ionization energy, the lower the electronegativity

Question 25

Alkali Metals (IA)

Answer 25

classic physical properties of metals but with lower densities, one lose e- in valence shell, low Zeff value, large atomic radii, considered an active metal

Question 26

Alkaline Earth Metals (IIA)

Answer 26

higher effective nuclear charges than IA and smaller atomic radii, two e- in valence shell, considered an active metal

Question 27

Chalcogens

Answer 27

eclectic group of nonmetal and metalloids, crucial normal biological functions, six e- in valence shells, small atomic radii and large ionic radii

Question 28

Halogens

Answer 28

highly reactive nonmetals with seven valence e-3, high electronegativities and electron affinities, reactive towards alkali and alkaline

Question 29

Noble Gases

Answer 29

aka “inert gases”, minimal chemical reactivity due to filled valence shells, high ionization energy, no measurable electronegativities

Question 30

Transition Metals

Answer 30

low electron affinities, low ionization energies, and low electronegativities, very hard, high melting and boiling points, malleable, good conductors