Periodic Table

Question 1

Father of the Periodic Table

Answer 1

Mendeleev

Question 2

Chemistry of a group #1

Answer 2

1. elements in a group have similar chemical properties because the have the same # of valence electrons

Question 3

Chemistry of a group #2

Answer 3

2. group elements form similar compounds

Question 4

Chemistry of a group #3

Answer 4

3. periodic table is arranged according to the atomic number (number of protons = nuclear charge)
   Trend: increases as you move down the group

Question 5

Chemistry of a group #4

Answer 5

4. atomic radius: distance between the nucleus and the farthest electron
   Trend: atomic radius increases as you go down the group because more occupied rings, create a greater distance between the atom’s nucleus and its furthest electron

Question 6

Chemistry of a group #5

Answer 6

5. first ionization energy: the amount of energy needed to remove the most loosely bound electron from the valence shell (measures hoe easy/hard an atom loses electrons)
   Trend: I.E decreases as you go down a group because atoms with larger radius have valence electrons that are farther away from their nucleus, so its easier to lose electrons

Question 7

Chemistry of a group #6

Answer 7

6. electronegativity: a measure of the attraction of a nucleus of one atom for another atom’s valence electrons
   Group Trend: decreases as you go down the group because atoms with a big radius, have a low en. attraction for another atom’s electrons decreases with more occupied rings, because it’s nucleus is further from another atom’s valence shells.

Question 8

Chemistry of a group #7

Answer 8

Metallic Property: measure of how easily an element loses electrons
Trend: the metallic properties increases as you go down the group; lose electrons easily because elements on the bottom of the group have low I.E and low E.N, so they lose electrons very easily/ react easily

Question 9

Group 1

Answer 9

alkalai metals: extremely active, form strong bases

Question 10

Group 2

Answer 10

alkaline earth metals: very active, but not as much as alkalai metals

Question 11

Properties of group 1 and 2

Answer 11

• found only in compounds in nature
• most active metals on the table
• lose electrons easily bc of low ionization energy and electronegativity
• form only ionic compounds
• form stable compounds (hard to decompose )
• group 1 elements are more active than group 2
• as the atomic # increases, elements become more active (more metallic; Low IE and Low EN)

Question 12

group 3 - 12

Answer 12

transition metals
- have multiple oxidation numbers (ex. cu can lose 1 or 2 electrons)
- can form compounds which have colored ions in water (ex. CuSO4 - blue)
- some transition elements are found commonly in the elements from nature (ex. Au, Cu, Ag)
- Hg is the only liquid at room temp

Question 13

group 13

Answer 13

borons family

Question 14

group 14

Answer 14

carbons family

Question 15

group 15

Answer 15

nitrogens family

Question 16

group 16

Answer 16

oxygens family

Question 17

group 17

Answer 17

halogens (non metals) - all halogens have 7 valence electrons (gain 1 electron to become -1 ions)

Question 18

bromine

Answer 18

liquid at room temp

Question 19

iodide

Answer 19

solid at room temp

Question 20

group 15, 16, 17 have

Answer 20

high electronegativity (gain another atoms electrons easily); high ionization energy (do not lose their electrons easily)

Question 21

group 18

Answer 21

noble gases: all are non metals and gases at room temp
- do not react with other elements bc they have filled/stable outer shell

Question 22

More protons pull electrons closer to the nucleus and atomic radius decreases

Answer 22

just know this info

Question 23

Characteristics of a period

Answer 23

• elements in the same period:
• number of occupied PEL’s are the same (ex. period 3 elements all have 3 occupied rings)
• as one moves across a period
  1) atomic number increases
  2) number of valence electrons increases
  3) atomic radius decreases: energy levels are kept closer to the nucleus, bc of a greater nucleus charge

Question 24

Across a period ionization energy increases because..

Answer 24

it takes more energy to remove electrons from non-metals (right side ) than metals (left side); non-metals are more attracted to their electrons because greater nuclear charge causes electrons to be held closer to the nucleus due to smaller radius

Question 25

across a period electronegativity increases because..

Answer 25

the attraction for another atom's electrons increases (atomic radius decreases; atoms nucleus is closer to another atoms valence electrons) because of a greater nucleus charge since the distance between that atoms nucleus and another atoms electrons decreases

Question 26

Metals

Answer 26

- have luster (shine ); mobile electrons - ductile - malleable - good conductor of electricity and heat - all are solids at room temp, except Hg - lose electrons become (+) ions - ionic radius is smaller than atom radius low I.E and low E.N - Fr is the most reactive metal

Question 27

Non Metals

Answer 27

- found on the right of the staircase - most are gases; some are liquids - Br is the only liquid non-metal - I is a solid non-metal at room temp - F is the most reactive non - metal - Lack luster; have a dull surface - not malleable or ductile; tend to be brittle - poor conductors of electricity or heat - non metals gain electrons become (-) ions - ionic radius is larger than atomic radius

Question 28

Metalloids

Answer 28

semi metals - elements at the staircase between the metals and non-metals - have some properties of both metals and non - metals - ex. malleable, bad conductors - 6 metalloids to know are B, Si, As, Te, Ge, Sb

Question 29

Kr and Xe

Answer 29

have some chemical reactivity

Question 30

Si

Answer 30

Metalloid

Question 31

which group contains elements in 3 phases at STP

Answer 31

halogens

Question 32

which halogen is solid at STP

Answer 32

iodide

Question 33

why is sulfur considered a group 16 element?

Answer 33

because an atom of sulfur has 6 valence electrons

Question 34

Which group 18 element can form a compound with fluorine

Answer 34

whichever one has the lowest ionization energy

Question 35

6 metalloids to know

Answer 35

B, Si, As, Te, Ge, Sb

Question 36

colored ions are which group

Answer 36

transition metals (3-12)

Question 37

what two elements are liquid at STP

Answer 37

Hg and Br

Question 38

What occurs when an atom loses an electron

Answer 38

the atoms radius decreases and the atom becomes a positive ion

Question 39

which group are monoatomic gases

Answer 39

group 18

Question 40

a magnesium atom that loses two electrons becomes a

Answer 40

positive ion with a smaller radius because its losing electrons so the radius becomes smaller

Question 41

lewis dot- structure

Answer 41

only contains valence electrons

Question 42

when metals form ions they tend to do so by

Answer 42

losing electrons and forming positive ions

Question 43

metalloids have

Answer 43

properties of metals and non-metals