• No results found

Ch 6 notes.ppt

N/A
N/A
Protected

Academic year: 2020

Share "Ch 6 notes.ppt"

Copied!
70
0
0

Loading.... (view fulltext now)

Full text

(1)

Bellwork

Monday, 10/29

To the right is

a label from a

popular food

item. Name

five elements

that are

found on this

food label.

I have the test graded I will show you the grades once the we finish

(2)

Test scores:

Lab Test WS 1st Period

(3)

CHEMISTY I

CHAPTER 6

(4)

Molecule- the smallest electrically

neutral unit of a substance that still

has the properties of that substance

-made up of two or more atoms that

act as a unit Ex.

H

2

O

CH

4

O

2

CO

2

(5)

Molecular

compound-

-usually composed

of molecules

-Have

low melting

& boiling points

-Are usually made

up of two or more

NONMETALS

Sugar, a compound made of carbon, hydrogen and oxygen, melts easily in a hot pan.

(AKA: Covalent)

Which of the following are molecular compounds? H2SO4 Pb(NO3)2

(6)

Which of the following is molecular

and which is ionic?

•NaCl

•H

2

O

•CaCO

3

•CO

•Al

2

Cl

3

•CF

4

•O

3

Hint: If it is not

(7)
(8)

triatomic

molecule- contain

three atoms of

the same element

(9)

Molecular Compounds and Acids

Binary Molecular Compounds

When naming binary molecular compounds,

prefixes are used to tell how many of each atom is in the formula.

CO2 carbon dioxide

(10)

The prefix mono- is never used with the first element. The prefix list in on page 159.

1- 6-2- 7-3- 8-4- 9-5- 10-mono tri tetra nona octa hepta penta hexa deca di

What prefixes would you use to describe a compound with four carbons and 10

(11)

Example:

 phosphorous tribromide

ICl3

P2O5

SF6

tetraarsenic hexoxide

PBr3

iodine trichloride

diphosphorous pentoxide

Sulfur hexafluoride

(12)

Acids and Bases

You need to know the names and

formulas of these most common acids:

HCl

H2SO4

HNO3

HC2H3O2

H3PO4

hydrochloric acid sulfuric acid

nitric acid acetic acid

(13)
(14)

Ions-

atoms or groups of atoms

that have a positive or negative

(15)

Let’s Practice!

Sodium loses an electron Na  __________

Magnesium loses two electrons Mg  __________

Chlorine gains one electron Cl  __________

Phosphorus gains three electrons P  __________

Na2+

Mg2+

Cl

-P3+

Atom “X” loses one

electron. What is its new charge?

(16)

Cation-

-positively charged ion -electrons were lost

-metals tend to form cations

-name of monatomic cation is the same as the element

We are positive about

(17)

Examples:

Na  Na+ + e

-Ca  -Ca2+ + 2e

(18)

-Anion

-

negatively charged ion -electrons were gained

-nonmetals tend to form anions

-name of monatomic anion ends in –ide

Cl + e-  Cl -O + 2e-  O 2-N + 3e-  N

3-Examples:

We feel negatively about ants!

Classify the following as cations or anions. H+ ___________

K+ ___________

F- ____________

C+4 ___________

(19)

Bellwork, Tuesday

How many protons, neutrons and electrons are in this atom?

Based on what you know about the charge of a proton and an electron, what is the overall charge of

this atom? What element is this atom?

Red =protons

(20)

Ionic

compound--composed of cations and anions

-usually metal & nonmetal -electrically neutral

-mostly solids at room temperature

-high melting points

-the more positive element always comes first

(21)
(22)

Monatomic Ions

The charge of a monatomic ion can often be determined by the element’s position on the periodic table:

Group 1A: 1+ Ex. Na+

Group 2A: 2+ Ex. Ca2+ Group 3A: 3+ Ex. Al3+ Group 5A: 3- Ex. N

3-Group 6A: 2- Ex. O

2-Group 7A: 1- Ex. F

(23)

Alkali metals have a charge of +1

Alkaline Earth metals have a charge of +2

The boron family has a charge of +3

The carbon family has a charge of + or -4

The nitrogen family has a charge of -3

The oxygen family has a charge of -2

The halogens have a charge of -1

The noble gasses have no charge and are inert

Transition

(24)

Elements in Group 0 (8) do not form

ions. Elements in Group 4 rarely form ions. They tend to react by sharing

electrons (forming covalent

compounds) instead of transferring electrons.

Group 8 Electron configuration = s2p6

(25)

What causes the charges for each group on the periodic table?

The charges indicate how many electrons an atom will gain or lose.

(26)

Octet Rule and Stabi

lity

The goal of an atom is to become stable. An atom will gain, lose, or share electrons in order for that stability to be attained.

Stability is determined by the octet rule:

(27)

• Ex: Potassium (and all of group 1) has 1 valence electron, so it will lose 1 electron making its charge +1.

Remember that electrons are

(28)

Examples: OPFNaMgAl

Sr 2+

(29)

Transition Metal ions (See Table 6-3 pg 144):

Most transition metals form more than one ion. They are stable losing

varying numbers of electrons. The

(30)

Exceptions:

(31)

What is the formula for the

following transition metals as ions?

Copper (I)

Iron (III)

Lead (II)

(32)

The mercury(I) ion is unique. It only exists in pairs of mercury(I) ions (like Siamese twins). Its

(33)

Quick Check Quiz: Have you been studying your ions?

sodium _______ chromous ________

selenide _______ tin(IV) ________

Na

+

Cr

2+

Se

(34)

Rubidium loses one electron _____

Silver loses one electron _____

Arsenic gains three electrons _____

Sulfur gains two electrons _____

Lithium loses one electron _____

Tuesday Bellwork

(35)

Wednesday Bellwork

Name the following compounds or

write the formulas, as appropriate.

CCl

4
(36)

Thursday Bellwork

Practice your ions! Write the symbol and charge for the following ions.

Nitride

Oxide

Magnesium ion

Rubidium ion

(37)

Friday Bellwork

Match the following ions with their names. ___NO3- A. nitride

___CN- B. silver ion

___Ag+ C. cyanide

___NH4+ D. ammonium

___N3- E. chloride

(38)

Polyatomic Ions

(Table 6-4, pg 147):

-tightly bound groups of atoms that behave as a unit and carry a

charge

(39)

The only positively charged

polyatomic ion that we need to

(40)

Ions that end in –ite or –ate contain

oxygen. In a series such as sulfate and sulfite, the –ite ending has one less

oxygen than the –ate ending.

Sulfite SO3

(41)

2-SO32- sulfite

SO42- sulfate

NO2- nitrite

(42)

Binary compounds- 2 elements Binary ionic compounds-

1 metal + 1 nonmetal

(43)

Examples:

NaCl

NaF

CaCl2

metal nonmetal

(44)

When naming ionic compounds,

simply name the ions as they appear in the formula.

When naming ionic compounds

(45)
(46)
(47)

Example:

AlCl3KBr FeCl2 FeCl3

aluminum chloride potassium bromide iron(II) chloride

(48)

When writing the formula for an

ionic compound, the charges of the ions must cancel out to give the

(49)

Example:

sodium chloride

Na

+

Cl

-1 1

(50)

magnesium iodide

Mg2+ I

-1 2

(51)

magnesium nitride

Mg 2+ N

3-2 3

(52)

strontium selenide

Sr2+ Se

2-2 2

(53)

rubidium iodide

aluminum oxide

Rb+ I

-RbI

Al3+

O

(54)

When writing formulas containing

polyatomic ions, use parentheses around multiple polyatomic ions.

ammonium carbonate

NH4+ CO 3

2-2 1

(55)

strontium hydroxide

Sr2+ OH

-1 2

(56)

calcium nitrate

Ca2+ NO 3

-1 2

(57)

aluminum phosphate

Al3+ PO

4

3-3 3

(58)

Monday Bellwork

Practice this ion quiz:

NO3- _______________________

Mercury (II) _______________________

Ag+ _______________________

CN- _______________________

Potassium _______________________ Bromide _______________________

(59)

When naming ionic compounds

containing a transition metal, don’t forget to include the Roman

numeral for the charge.

Ex. FeCl2

iron(II) chloride FeCl3

(60)

Distinguish Between the

two types of compounds!

Molecular

Ionic

•Two or more nonmetals

Low melting pointLow boiling point •Example CO2

•Metal and nonmetals

High melting pointHigh boiling point

Solid at room temperature •Electrically neutral

(61)

Which of the following is molecular and which is ionic?

NaBr

CO2

O3

NO

KCl

AlBr3

(62)

Chemical formula- shows the number and kinds of atoms in the smallest

representative unit of the substance.

Molecular formula- chemical formula

written for a molecule

Ex. CO

2

O

2

or H

2

O

2
(63)

Formula unit- chemical formula

written for an ionic compound.

(64)

Tuesday Bellwork

Name the following compounds.

NaBr _____________________________

Al(OH)3 ___________________________

NH4F _____________________________

Li2SO3 ____________________________

CaBr2 ____________________________

KMnO4 ___________________________

Fe(NO3)2__________________________

(65)

Law of Definite Proportions-

In all samples of any chemical compound, the elements are always combined in the same proportion by mass.

(66)

Law of Multiple Proportions- Whenever two elements form more than one

compound, the different masses of one element that combine with the same

(67)
(68)

Wednesday Bellwork

 Using the food label shown, write two

(69)

Thursday Bellwork

Write the formulas for these compounds.

 Potassium chlorite

 Calcium hydrogen carbonate

 Dichlorine heptoxide

 Trisilicon tetranitride

 Sodium dihydrogen phosphate

(70)

Friday Bellwork

References

Related documents

Other variable renewable energy technologies are also likely to see improvements, but not to match the expected capacity factors of new offshore wind projects [11,12,13,14]. For

It is also one of the most costly diseases Mastitis, the most important deadly disease of dairy animals is responsible for heavy economic losses due to reduced milk yield

Medium supplemented individually with auxins and cytokinins induced formation of shoots and among the various concentrations, BAP (1.0 mg/l) was proved to be optimum for

This, it is contended, is an example of how iconic positioning and strategy can be authentic – not only in its’ brand design, brand development, and brand strategy – but also in

Im- proved understanding of such scenarios might lead to re- finements in the diagnosis and treatment of ophthalmic diseases where central vision is impoverished while pe-

which on average occur once every 50-120 years somewhere in Utah and once every 300-400 years on the Wasatch fault in the urban Wasatch Front area (last large earthquake in Utah was

We wished to determine the potential for MSC therapy to exert beneficial effects in the early recovery phase following VILI when ongoing injury coexists with processes of repair, and

Emergency medicine and critical care Ultrasound is becoming an indis- pensable diagnostic tool in the emer- gency department (ED) and the inten- sive care unit (ICU), as urgent