11th Chemistry - Chpt 6 & 7

Question 0

Define group/family/column

Answer 0

Group/ Family - 18 columns of elements in periodic table

Question 1

Define period and row

Answer 1

Period/Row. - 7 rows of elements in periodic table

Question 2

How is the periodic table organized?

How does atomic number change as you move around in the table (L/R and up/down)?

Answer 2

Rows - increasing atomic number as you move left to right

Columns - increasing atomic number as you move down

Question 3

In the periodic table what is the general location of the
Metals
Metalloids
Non-metals

Answer 3

Metals - left side
Metalloids - middle diagonal
Non-metals - upper right

Question 4

What are the properties of alkali metals?

Answer 4

• group 1
• very reactive
• usually found in compounds (i.e. Table salt,)

Question 5

What are the properties of halogens?

Answer 5

• group 17

- Usually found in compounds

Question 6

What are the noble gases?

Answer 6

• group.18

- Extremely unreactice

Question 7

How do you count valence electrons?

What impact does it have on Bohr diagrams?

Answer 7

2/6/16

Determines how many electrons are in the outer ring

Question 8

What are Lewis structures?

Answer 8

Dots around element symbol show number of valence electrons. Max of 8

Question 9

What is the Octet Rule?

Answer 9

Elements will try to stabilize by getting 8 electrons in the outer ring

Elements on right side of periodic table tend to gain electrons and form (-) electrons

Elements on left side of periodic table tend to lose electrons and form (+) ions

Question 10

What is an ion? When would it have a positive charge? When would it have a negative charge?

Answer 10

Ion is an atom with either one extra/one less electron than the base element?
One less - positive charge- cation
One more - negative charge - anion

Question 11

What is the atomic radius?

Answer 11

atomic radius is one-half the distance between the nuclei of two atoms

• decreases from left to right within a period.
  increase in the number of protons draws electrons in
• increases from top to bottom within a group

Question 12

What is the ionic radius?

Answer 12

Positive ions (missing electron) - smaller. Drawn into + center

Negative ions (added electron) - larger. Push away from + center

Question 13

What is ionization energy?

Answer 13

Energy used to hold onto electrons
-higher ionization energy holds electrons more tightly
- higher ionization energy less likely to lose an electron and develop
(+) charge
- ionization energy generally increases from left to right. This is due to valence shell stability.
- ionization energy within a group generally decreases from top to bottom.
- noble gases possess very high ionization energies because of their full valence shells
- helium has the highest ionization energy

Question 14

What is electronegativity?

Answer 14

Indicates relative ability of element atoms to ATTRACT electrons in a chemical bond. ElectroNEGATIVITY

Decreases as you go Down the table
Raises as you go Right in the table
Noble gases are 0

Question 15

What are periodic trends?

Electronic summary assignment & PP notes

Answer 15

Period and group trends in atomic radii are related to electron configuration ???

As atomic radius grows - # protons grows -
# electrons grows
- so more rings 2/10/18/26 etc

Question 16

Atoms with large ionization energy values are _________.
A. More likely to form positive ions
B. Less likely to form positive ions
C. Most likely to lose their outer electrons
D. Lacking valence electrons

Answer 16

B. Less likely to form positive ions

Question 17

Which of the following is an ion?
A.  O2-
B.  C
C   HCI
D.  LI-3

Answer 17

A. O2

Question 18

Where on the periodic table would you expect to find the smallest atoms? 
A. Upper left
B. Upper right
C. Lower left
D. Lower right

Answer 18

B. Upper right

Question 19

Why are ionic radii generally larger for group 15 than for group 17?
A. Atoms in group 15 are larger than atoms in group 17
B. Atoms in group 15 have more protons than atoms in group 17
C. Ions of group 15 have greater negative charge than ions of group 17 atoms
D. Atoms in group 15 are generally more electronegative than atoms in group 17

Answer 19

C. Ions of group 15 have greater negative charge than ions of group 17 atoms

Question 20

Is ionic radius smaller or larger for a positive ion?

Answer 20

Smaller. + charge. Drawn into + center

Question 21

T/F

Ionic radius of both positive and negative ions gets larger as you move down a group

Answer 21

True.

Question 22

T/F

Generally, ionic radius gets smaller as you move right on the periodic chart

Answer 22

True.
+ ions decrease in groups 1-14
- ions decrease in groups 15-17.

Question 23

T/F

The periodic table organizes the elements by atomic mass

Answer 23

False

By atomic number

Question 24

T/F | The periodic table organizes elements into periods(columns) and groups our families (rows)

Answer 24

False periods - rows groups or families- columns

Question 25

The correct match of elements to group is: A-alkali metals B-halogens 1- group 18. 2- group 1 C-alkaline earth metals D- noble gases. 3- group 2. 4- group 17 A. A-1. B-3. C-2. D-4 B. A-3 B-2. C-1. D-4 C. A-2 B-4. C-3. D-1 D. A-4. B-1. C-2. D-3

Answer 25

C. A-2 B-4. C-3. D-1

Question 26

``` Elements in the same group of the periodic table have the same_______? A. Number of valence electrons B. Physical properties C. Number of electrons D. Electron configuration ```

Answer 26

A. Number of valence electrons

Question 27

``` On the modern periodic table, metalloids are found only in _________. A. Groups. 3-5 B. Groups 13-17 C. Group 18 D. Groups 1-2 ```

Answer 27

B. Groups 13-17

Question 28

``` Which group is composed entirely of nonmetals? A. 1 B. 13 C. 15 D. 18 ```

Answer 28

D. 18. Noble gases

Question 29

T/F | Nitrogen has the highest ionization energy of all the elements.

Answer 29

False | helium has the highest ionization energy of all the elements.

Question 30

T/F | The noble gases possess very high ionization energies because of their full valence shells.

Answer 30

True. All group 18 elements have full valence shells. 2/10/18/26/34/42 etc helium has the highest ionization energy of all the elements. Shell of 2 electrons

Question 31

Which correctly describes elements in the same family? A. Same number of valence electrons B. Electrons in the same outermost energy level C. Same atomic radius D. Must be in same state of matter

Answer 31

A. Same number of valence electrons

Question 32

``` Elements with the physical and chemical properties of both metals and non-metals are A. Radioactive metals B. Transition metals C. Metals or semi-metals D. Gaseous metals ```

Answer 32

C. Metals or semi-metals

Question 33

``` Most atoms that form ions become more stable by following the___________ rule, which means there will be _____ electrons in its outermost layer A. Triplet- 3 B. Octet- 4 C. Duet - 2 D. Octet - 8 ```

Answer 33

D. Octet - 8

Question 34

``` An atoms ability to attract electrons is its A. electronegativity B. Heat of reaction C. Ionization energy D. Heat of formation ```

Answer 34

A. electronegativity

Question 35

``` Which property describes h how much energy must be added to an atom to remove an outermost electron? A. Atomic radius B. Electronegativity C. Ionic radius D. Ionization energy ```

Answer 35

D. Ionization energy

Question 36

``` Which group contains the most unattractive and stable elements? A. 1 B. 2 C. 17 D. 18 ```

Answer 36

17

Question 37

``` Which family contains the halogen family of elements? A. 1 B. 2 C. 17 D. 18 ```

Answer 37

C. 17

Question 38

A cation is an element which has gained an electron?

Answer 38

False. Lost (-) electron and is now(+)

Question 39

What is an ionic computed? | Why does it not have an overall charge?

Answer 39

???