Unit 6 test

Question 1

Metal

Answer 1

shiny
ductile
malleable
good conductors
solid
lose valence electrons

Question 2

Nonmetal

Answer 2

mostly gases,
poor conductors
gain electrons

Question 3

Metalloid

Answer 3

semi condictors, in between properties of metals and non-metals

Question 3

Malleable

Answer 3

easily shaped or formed

Question 4

Ductile

Answer 4

stretched or bent without breaking

Question 5

Periods

Answer 5

1-7 on a periodic table

Question 6

Periodic Law

Answer 6

when elements are arranged according to increasing atomic number there is periodic repition of their chemical and physical properties

Question 7

Noble Gases

Answer 7

unreactive, no need to gain electrons very stable

Question 8

Inert

Answer 8

chemically inactive

Question 9

Halogens

Answer 9

very reactive
tend to gain 1 electron in reactions
low melting and boiling points
toxic

Question 10

Alkali Metals

Answer 10

very reactive,
high boiling & melting points
lose 1 electron in reaction

Question 11

Alkaline Earth Metals

Answer 11

silvery white
high boiling point
lose 2 electrons

Question 12

Main Group Elements

Answer 12

groups 1-2 and 13-18

Question 13

Transition Metals

Answer 13

groups 3-12

Question 14

Cation

Answer 14

atom with a postive charge (+)

Question 15

anion

Answer 15

atom with negative charge (-)

Question 16

Which elements are unreactive or inert?

Answer 16

nobel gases becasue they have a full outer shell

Question 17

What does it mean to describe something as periodic

Answer 17

repeating or regular pattern of properties that elements exhibit when arranged in order of increasing atomic number.

Question 18

What kind of important information is represented by the period numbers?

Answer 18

the number of electron shells (or energy levels) that the elements in that row have.

Question 19

What are the only two liquid elements? Which one is a metal?

Answer 19

mercury (metal)
bromine (halogen)

Question 20

How many electrons are in Mg2+? In S2-?

Answer 20

+2 means the atom lost 2 electrons giving it an postive and visversa

Question 21

Describe the periodic trend for atomic size down a group and across a period.

Answer 21

Big-Small
Small
I
Big

Question 22

What causes ionization energy to decrease going down a group?

Answer 22

The outer electrons are farther from the nucleus, so it’s easier to remove them. Inner electrons block the attraction between the outer electrons and the nucleus, making it easier to remove an electron.

Question 23

What causes ionization energy to increase going across a period?

Answer 23

the atoms get smaller and the nucleus holds the electrons more tightly

Question 24

What makes a metalloid like silicon a good material for computer chips?

Answer 24

semi conductor properties

Question 25

List all the metalloids:

Answer 25

Boron (B)
Silicon (Si)
Germanium (Ge)
Arsenic (As)
Antimony (Sb)
Tellurium (Te)
Polonium (Po)

Question 26

What is another name for the represtentative elements

Answer 26

main group elements

Question 27

why is cation and anion smaller and larger then the atom it came from

Answer 27

cation is smaller - loses. With fewer electrons, the remaining electrons are pulled closer to the nucleus, making the ion smaller.
anion is larger - gains. The added electrons increase repulsion between them, causing the electron cloud to spread out, making the ion larger.

Question 28

why atomic size increases down a group

Answer 28

as you go down a group, atoms have more layers of electrons, making them bigger.

Question 29

ionization energy

Answer 29

the energy required to remove an electron from an atom.

Question 30

why does ionization energy have the trend

Answer 30

atoms are smaller and more tightly held, and it decreases down a group because atoms are larger and the electrons are easier to remove.

Question 31

electronegativity

Answer 31

the ability of an atom to attract and hold onto electrons when it forms a bond with another atom.

Question 32

WHY the trend for atomic radius within a period is the way it is.

Answer 32

the increasing nuclear charge pulls the electrons closer, causing the atomic radius to decrease.