Chapter 5

Question 1

rValence electrons

Answer 1

an electron that is found in the outermost shell of an atom
determines the atoms’s chemical properties

Question 2

period

Answer 2

same row, same number of occupied energy levels

Question 3

group

Answer 3

elements share chemical properties vertical columns

Question 4

main group elements

Answer 4

The s and p block

Question 5

ionization energy

Answer 5

amount of energy needed to remove

Question 6

electronegativity

Answer 6

a measure of the ability of an atom

Question 7

electron sheilding

Answer 7

the reduced attraction between positively charged nucleus and negatively charged valence electrons

Question 8

effective nuclear charge

Answer 8

the amount of positive charge that actually acts on an electron

Question 9

atomic radius

Answer 9

half the distance

Question 10

periodic law

Answer 10

the physical and chemical properties

Question 11

periodic table

Answer 11

an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column or group

Question 12

ionic radius

Answer 12

1/2 the distance from center of two connected ions

Question 13

trend

Answer 13

predictable change in a particular direction

Question 14

periodic trend

Answer 14

generalizations about atoms and their properties

Question 15

alkali metals

Answer 15

group 1
react strongly with water
combine rigorously with nonmetals
usually stored in kerosene or mineral oil
soft, cut with a knife

Question 16

alkaline earth metals

Answer 16

group 2
less reactive than alkali and are found as compounds
harder, denser, stronger than alkali metals
pair of electrons in outermost sublevel
loses 2 electrons to become stable

Question 17

transition metals

Answer 17

Groups 3-12
good conductors of electricity
less reactive than groups 1 and 2
high luster (shiny)

Question 18

halogens

Answer 18

group 17
highly reactive
react with metals to form salts
7 electrons in outermost energy level

Question 19

noble gases

Answer 19

group 18
8 electrons in outer energy level which make the gasses stable
unreactive
do not readily gain or lose electrons

Question 20

metalloids

Answer 20

semi conducting elements in p-block
between metals and non metals
mostly brittle solids
share properties of metals and nonmentals
ON THE STAIRCASE

Question 21

lanthanides

Answer 21

f block top
called rare earth metals
reactive like group 2
shiny metals
used in Tv’s magnets and lasers

Question 22

Actinides

Answer 22

f block bottom
atomic numbers 90-103
All are radio active
first four found naturally while others are made in a lab
uranium is used to produce nuclear power
some elements are so unstable they exist for only a fraction of a second

Question 23

cation

Answer 23

positively charged ion; loss of e-

Question 24

anion

Answer 24

negatively charged ion; gain of an e-

Question 25

what are the main group of elements located?

Answer 25

s and p blocks

Question 26

what do elements in the same period have in common

Answer 26

same number or occupied energy levels

Question 27

what do elements in the same group have in common

Answer 27

share chemical properties

Question 28

are elements with similar chemical properties more likely to be found in the same period or in the same group? why?

Answer 28

Same group because they have the same number of valance electrons which means they share chemical properties

Question 29

what group of elements easily gains one valence electron

Answer 29

halogens all elements want to have the most valence electrons which is 8

Question 30

why are the alkaline earth metals less reactive than the alkali metals

Answer 30

they are further inward on the periodic table

Question 31

who is credited with organizing the original periodic table

Answer 31

Mendeleev

Question 32

How was Mendeleev's periodic table organized

Answer 32

atomic mass

Question 33

how is the modern day periodic table organized

Answer 33

atomic number

Question 34

ion

Answer 34

atom or molecule that has gained or lost electrons

Question 35

atomic radius trends

Answer 35

increase as you go down more e- causes more energy levels for e- smaller as you move from left to right across a period more p+ means stronger pull on outermost electrons

Question 36

ionic radius trends

Answer 36

increases as you move down a column more energy levels for e- larger ions decreases as you move left to right across a period more p+ means stronger pull

Question 37

ionization energy trends

Answer 37

decreases as you move down a group more e- shielding increases as you move left to right across a period elements want to gain e- not lose e-

Question 38

electronegativity trends

Answer 38

decreases as you move down a group more e- shielding increases as you move left to right across a period noble gases are stable