Chemistry Unit 4 Review

Physical Properties

100

the distance from the nucleus to the outermost shell

atomic radius

200

atomic radius decreases from left to right on periodic table because: 

the number of protons increases, pulling all the electrons in closer to the nucleus

300

atomic radius increases from top to bottom in a group because: 

number of shells increase as you go down group; more shells = larger radius

400

when core electrons prevent valence electrons from being pulled in by the nucleus, this is called: 

shielding/shield effect

500

the distance from nucleus to outer shell of an ion

ionic radius

More Physical Properties

100

the radius of a cation of an element is ___________ than the neutral atom of that element because it loses electrons

smaller

200

the anion of an element is __________ than the neutral atom of that element because it gains electrons

larger

300

which of the following has the largest radius: 

Rb, Rb⁺, Sr²⁺, Be

Rb

400

which of the following has the largest radius: 

Se, S, S^2-, Se^2-

Se^2-

500

atomic radius is measured in this unit

Angstrom, Å

Oxidation States

100

group 17 has this charge when it ionizes

1-

200

the alkali metals all have  this charge when they ionize

1+

300

this group has an oxidation state of 3- when it ionizes

group 15

400

all the elements in group 2 have this oxidation state

2+

500

the oxidation state of sulfur is: 

2-

Chemical Properties

100

these electrons are responsible for chemical bonding

valence electrons

200

the electrons responsible for shielding/shield effect

core electrons

300

the energy required to remove an electron from an atom

ionization energy

400

the energy released when an atom gains an electron

electron affinity

500

the measure of the strength with which an atom pulls on shared electrons is called:  

electronegativity

More Chemical Properties

100

On periodic table, electronegativity increases 

bottom L to top R

or

L-->R, bottom to top

200

on periodic table, electron affinity increases: 

bottom L to top R

300

on periodic table, ionization energy increases: 

bottom L to top R

400

Ionization energy and electron affinity are measured in this unit

electron volt (eV)

500

Ionization energy increases in the same direction as electron affinity and electronegativity because: 

the more tightly an atom holds onto electrons (the more it wants electrons) the more energy it will take to remove the electrons