Chemistry (Periodic Table)

Front 1

mendeleev

Back 1

noticed that there were patterns in reactivity, size,physical properties. ordered the periodic table by atomic mass

Front 2

mosely

Back 2

ordered periodic table by atomic number

Front 3

groups

Back 3

columns (families )

Front 4

group 1

Back 4

Does not include H
alkali metals

Front 5

group 2

Back 5

alkaline earth metals

Front 6

group 3-12

Back 6

transition metals

Front 7

bottom 2 rows

Back 7

inner transition metals

Front 8

group 17

Back 8

halogens

Front 9

group 18

Back 9

includes helium
noble gases

Front 10

what do the group's have in common

Back 10

the same number of valence electrons

Front 11

metals

Back 11

left of staircase
doesn't include H

Front 12

nonmetals

Back 12

right of staircase
liquids:Br
solids: C, P, Se, I, S
gases: H,N,O,F,Cl group 18

Front 13

metalloids

Back 13

on the staircase

Front 14

allotropes

Back 14

different forms of same element

Front 15

metals:physical properties

Back 15

1. luster
2. good conductivity: heat, electricity, carries heat and electricity from On spot to another
3. malleable- Bend into sheets
4. ductile: mold into wires

Front 16

nonmetals

Back 16

1. dull
2. good insulators -hold in heat
3. brittle

Front 17

lewis dot diagrams for atoms/ions

Back 17

Front 18

how does an atom become a cation

Back 18

decrease in radius
lose electrons
metals do this

Front 19

how does an atom become an anion

Back 19

increase in radius
gain electrons
non metals do this

Front 20

atomic radius

Back 20

distance from nucleus to valence shell

Front 21

ionization energy

Back 21

energy needed to remove the most loosely held electron (valence shell )

Front 22

electronegativity

Back 22

attraction for an electron
noble gases don't have one

Front 23

down the group

Back 23

AR increases
IE DECREASES
EN DECREASES

Front 24

why does AR increase across a period

Back 24

# of energy levels increases (shells )

Front 25

down the group attraction

Back 25

the attraction decreases bc the distance increases, so less ionization energy is needed

Front 26

across a period

Back 26

AR DECREASES
IE INCREASES
EN INCREASES

Front 27

why does AR decrease across a period

Back 27

attraction gets stronger

Front 28

across a period

Back 28

-an increase in nuclear charge will increase the attraction for valence electrons
-effective nuclear charge increases so attraction increases so more IE is needed

Front 29

reactivity..metals lose electrons

Back 29

the bigger metals lose electrons more readily because the attraction decreases

Front 30

reactivity...nonmetals gain electrons

Back 30

the smaller gain electrons more readily because attraction increases

Front 31

group 1 metals are most..

Back 31

reactive (Fr is most)

Front 32

group 17 nonmetals are most

Back 32

reactive (F is most)

Front 33

alkali metals

Back 33

really reactive (esp with water )
not found in nature as elements
always in compound form
+ions (lose electrons react )

Front 34

alkaline earth metals

Back 34

-reactive (esp with water )
-not found in nature by itself always in compound form

Front 35

transition metals

Back 35

stable
building
multiple charges
colored solutions

Front 36

13,14,15,16

Back 36

nonmetal-metalloid-metal
*as you go down the periodic table metallic character increases*

Front 37

halogens

Back 37

group 17 diatomics
F2. (g )
Cl (g )
Br2 (l )
I2 (s )
-1 ions gain electrons

Front 38

noble gases

Back 38

monatomic
don't react valence shell is full