Chapter 6-Periodic Table

Question 1

Current periodic table is who’s model? What did he arrange the elements by?

Answer 1

Henry Moseley

atomic number

Question 2

each box of the periodic table has…

Answer 2

element name
symbol
atomic number
atomic mass

Question 3

period vs group

Answer 3

period: row
group: column

Question 4

Representative elements

Answer 4

s and p blocks

possess wide range of chemical and physical traits

Question 5

transition elements

Answer 5

d and f blocks

Question 6

metals

Answer 6

usually solid at room temp

good heat and electricity conductors

Question 7

Where are the metals located?

Answer 7

Left of staircase

Question 8

Malleability

Answer 8

ability to be pounded thin

Question 9

Ductility

Answer 9

ability to be drawn into wires

Question 10

alkali metals

Answer 10

group 1 elements

very reactive
usually exist as compounds with other elements

Question 11

alkaline earth metals

Answer 11

group 2 elements

very reactive

Question 12

transition elements divided into ___ and ___

Answer 12

transition metals and inner transition metals

Question 13

inner transition metals divided into ___ and ___, which are located in the ___ block

Answer 13

lanthanide series and actinide series

f block

Question 14

nonmetals located…

Answer 14

right of staircase

Question 15

nonmetals

Answer 15

usually gases or dull-looking solids

poor heat and electricity conductors

Question 16

which nonmetal is the only one that’s liquid at room temp?

Answer 16

bromine

Question 17

halogens

Answer 17

group 17

very reactive
often form compounds with other elements

Question 18

noble gases

Answer 18

group 18

Question 19

metalloids/semimetals

Answer 19

elements bordering staircase

physical and chemical traits of both metals and nonmetals

Question 20

only metal that is liquid at room temp?

Answer 20

Mercury

Question 21

counting valence e’s

Answer 21

look at s and p blocks (count in)

Question 22

noble gases have __ valence e’s each

Answer 22

8

Question 23

atomic radius

Answer 23

metals: 1/2 distance between a crystal’s adjacent nuclei
nonmetals: 1/2 distance between nuclei of identical atoms

Question 24

trend of atomic radii from left to right

Answer 24

decrease

# of protons increase from left to right
more protons have stronger pull on negative e's (increased positive charge on nucleus)
atoms become more constrained

Question 25

trend of atomic radii down a column

Answer 25

increase more energy levels although there are more e's, they're further away from the nucleus (less pull=less constraint)

Question 26

ion

Answer 26

formed when atom gains or loses e's

Question 27

ionic radius: lose electrons

Answer 27

becomes smaller e's lost (possible empty orbital) nucleus pulls remaining e's closer

Question 28

ionic radii trend: period (left to right)

Answer 28

positive ions decrease from groups 1-13 | neg ions decrease from groups 14-17

Question 29

ionic radii trend: groups

Answer 29

increases going down

Question 30

ionization energy

Answer 30

energy needed to remove valence e

Question 31

ionization energy trend in a period (left to right)

Answer 31

increases elements on right want to gain e's since they are closer to achieving the octet stronger pull

Question 32

ionization energy trend down a group

Answer 32

decreases atomic radius increases less pull

Question 33

octet rule

Answer 33

atoms tend to gain, lose, or share e's in order to get a full set of 8 valence e's

Question 34

electronegativity

Answer 34

ability to attract e's in a chemical bond

Question 35

types of ions

Answer 35

cation | anion

Question 36

cation

Answer 36

positive (lost e) metals smaller than original atom

Question 37

anion

Answer 37

negative, gain e nonmetals larger than original atom

Question 38

shielding

Answer 38

e's between nucleus and valence shell shield pull on valence e's

Question 39

ditomic elements

Answer 39

7, make a 7 in periodic table always occur in pairs in nature (ex. N2, O2) top of 7 starts at NOF

Question 40

periodic law

Answer 40

there's a periodic repetition of chemical and physical properties of elements when arranged by increasing atomic #

Question 41

shielding effect trend: period

Answer 41

constant

Question 42

shielding effect trend: group

Answer 42

increases from top to bottom more energy levels

Question 43

why are valence e's not shielded from the increasing positive nuclear charge as atomic radius increases across a period?

Answer 43

no e's (energy level n) come between the nucleus and valence e's

Question 44

second ionization energy

Answer 44

removing the 2nd e | requires more energy

Question 45

why is the octet rule useful?

Answer 45

used for predicting what types of ions an element will form

Question 46

Which block is He a part of?

Answer 46

s

Question 47

Why do elements in the same group have similar chemical properties?

Answer 47

same # of valence e's

Question 48

valence e configuration

Answer 48

last part of normal e configuration | shows the # of valence e's

Question 49

determining # of valence e's for representative elements

Answer 49

s and p block (count in)