Unit 3: Ionic and Metallic Substances Review - PowerPoint Presentation

Slide1

Unit 3: Ionic and Metallic Substances Review

Honors Chemistry

Slide2

1. Which of the following is ionic?

NF

3

HClCuCl2CO2

Slide3

2. Which of the following is covalent?

MgO

H

3NFeOZnCl

Slide4

3. To form an ion Nitrogen will

Lose 3 electrons to become N

3-

Lose 3 electrons to become N3+Gain 3 electrons to become N3-

Gain 3 electrons to become N

3+

Slide5

4. To form an ion K will

Lose 1 electron to become K

-

Lose 1 electron to become K+Gain 1 electron to become K-

Gain 1 electron to become

K

+

Slide6

5. What is the correct name for CaCl

2

?

calcium chloridecalcium dichloridemonocalcium dichloride

calcium (I) chloride

calcium (II) chloride

Need help with naming?

Watch this.

Slide7

6. What is the correct name for CuCl

2

?

copper chloridecopper dichloridemonocopper dichloride

copper (I) chloride

copper (II) chloride

Need help with naming?

Watch this.

Slide8

7. What is the correct name for

NaOH

?

sodium oxygen hydridesodium hydroxideSodium monooxygen monohydride

sodium (I) hydroxide

sodium (II) hydroxide

Need help with naming?

Watch this.

Slide9

8. What is the correct name for NH

4

Cl?

nitrogen tetrahydrogen chloridenitrogen (I) tetrahydrogen chloride

a

mmonium chloride

a

mmonium (I) chloride

Need help with naming?

Watch this.

Slide10

9. What is the correct name for FeC

2

H

3O2?iron carbon hydrogen oxideiron (I) carbon hydrogen oxide

Iron (I)

dicarbon

tri hydrogen dioxide

iron (I) acetate

Need help with naming?

Watch this.

Slide11

10. What is the correct formula for magnesium oxide?

Mg

2

O2MgOMgO2

Mg

2

O

Need help with naming?

Watch this.

Slide12

11. What is the correct formula for mercury (II) sulfite?

HgSO

3

HgSO4Hg2(SO3)

2

Hg(SO

3

)

2

Need help with naming?

Watch this.

Slide13

12. What is the correct formula for iron (III) oxide?

FeO

Fe

2O3Fe3O2

Fe(OH)

3

Need help with naming?

Watch this.

Slide14

13. What is true about electrons in ionic bonds?

Electrons are shared equally

Electrons are shared unequally

Electrons are transferred from the metal to the nonmetalElectrons are transferred from the nonmetal to the metal

Electrons move freely in in a “sea of electrons

Slide15

14. What is true about electrons in nonpolar covalent bonds?

Electrons are shared equally

Electrons are shared unequally

Electrons are transferred from the metal to the nonmetalElectrons are transferred from the nonmetal to the metal

Electrons move freely in in a “sea of electrons

Slide16

15. What is true about electrons in polar covalent bonds?

Electrons are shared equally

Electrons are shared unequally

Electrons are transferred from the metal to the nonmetalElectrons are transferred from the nonmetal to the metal

Electrons move freely in in a “sea of electrons

Slide17

16. What is true about electrons in metallic bonds?

Electrons are shared equally

Electrons are shared unequally

Electrons are transferred from the metal to the nonmetalElectrons are transferred from the nonmetal to the metal

Electrons move freely in in a “sea of electrons

Slide18

17. Why is it incorrect to call

NaCl

a molecule?

Molecules contain more than two atomsMolecules occur between a metal/nonmetalMany ions of Na+ and

Cl

-

exist in a crystal lattice

One ion of Na

+

and

Cl

-

have an ionic bond

The sodium ion forms a metallic bond with other sodium ions

Slide19

17. What is the general trend of electronegativity on the periodic table?

Electronegativity decreases as you move to the left and up

Electronegativity decreases as you move to the right and down

Electronegativity decreases as you move to the left and down

Electronegativity decreases as you move to the right and up

Slide20

17. Which is more electronegative, carbon, nitrogen, sulfur or phosphorus?

carbon

nitrogen

sulfurphosphorus

Slide21

18. Fill out this table with formulas

K

Ca

Cr (III)

Pb

(IV)

Br

CO

3

2-

N

PO

4

3-

Slide22

18. Fill out this table with formulas

K

Ca

Cr (III)

Pb

(IV)

Br

KBr

CaBr

2

CrBr

3

PbBr

4

CO

3

2-

K

2

CO

3

CaCO

3

Cr

2

(CO

3

)

3

Pb

(CO

3

)

2

N

K

3

N

Ca

3

N

2

CrN

Pb

3

N

4

PO

4

3-

K

3

PO

4

Ca

3

(PO

4

)

2

CrPO

4

Pb

3

(PO

4

)

4

Slide23

19.

For K

and S: a.) draw the electron dot structure b.) show the transfer of electrons to form ionsc.) draw the resulting ionsd.) write the formula of the compound they form

K

.

S

.

.

.

.

.

.

K

.

..

2K

+

+

S

2-

K

2

S

..

..

.

.