right side notes only title and highlight - chemistry ch 5.1-5.3 title and highlight draw any...

TN Ch 5.1-5.3 Date

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NOTES:

Write out the notes from my website.

Use different types of note-taking

methods to help you recall info (different

color pens/highlighters, bullets, etc)

When I lecture we will add more info, so

leave spaces in your notes

Summary Questions:

Write Book Question out and answer it

(in another color based on what you read

from my notes or textbook.

THESE ARE AT THE VERY END OF

NOTES

Right Side – NOTES ONLY

Reflect

Question:

Reflect on

the

material by

asking a

question

(its not

suppose to

be

answered

from

notes)

TN Ch 5.1-5.3

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DRAW ANY PICTURES, FIGURES,

AND WRITE OUT ANY PRACTICE

PROBLEMS/QUESTIONS.

WE WILL ANSWER THEM TOGETHER.

LEAVE SPACES SO WE CAN ANSWER

QUES.

LEFT Side – PICTURES, PRACTICE PROBLEMS, ETC

READ Ch 5.1-5.3 (pg. 127-132) first then take notes

Sodium chloride (NaCl) The properties of a compound are

different from the properties of the elements that compose it.

A few of the substances we encounter in everyday life are elements.

Majority are compounds or molecules.

In a compound, the elements combine in fixed, definite proportions. This is known as the Law of Constant Composition.

A chemical formula indicates the elements present in a compound and the # of atoms of each.

For example, H2O is the chemical formula for water; it indicates that water consists of H and O atoms in a 2:1 ratio.

The formula contains the symbol for each element with subscripts (little #’s) indicating the number of atoms of that element. (don’t write 1’s).

H2O1 = H2O

Common chemical formulas include: CO for carbon monoxide (1:1 ratio) CO2 for carbon dioxide (1:2 ratio). C12H22O11 for sugar (sucrose) (12:22:11 ratio).

If subscripts change, then the formula no longer is that compound. (Muy importante)

H2O vs. H2O2

CO (carbon monoxide), an air pollutant ◦When inhaled, CO interferes with the blood’s ability to carry oxygen, which can be fatal. ◦Called the “Sleep of death” gas

CO2 is carbon dioxide, produced from combustion and human respiration. We breathe small amounts of it all the time with no harmful effects….but harmful to the planet (aka global warming)!!!

1. Chemical formulas list the most metallic elements first.

Remember - Metals are on the left side of the P.T. and nonmetals on the upper right side. ◦The formula for table salt is NaCl, not ClNa.

2. In compounds that do not include a metal, the more metal-like element is listed first. (closest nonmetal to the staircase on P.T.)

3. Within a group in P.T. , elements toward the bottom are more metal-like than elements toward the top.

We write SO2 not O2S.

The specific order for listing nonmetal elements in a chemical formula is shown in Table 5.1

Left side!!!

Left side!!!

Some formulas contain groups of atoms.

Their formula is set off in parentheses with a subscript to indicate the number of that group.

Many of these groups of atoms have a charge associated with them and are called polyatomic ions. (Very important for the rest of year!! Hint, hint)

To determine the total number in a compound containing a group within parentheses, multiply the subscript outside the parentheses by the subscript for each atom inside the parentheses.

Determine the number of each type of atom in Mg(NO3)2.

Left side!!!

Practice Problem #3

Determine the number of each type of atom in the

following compounds.

(a) Al (C2H3O2)3

(b) Al2 (Cr2O7)3

(c) Pb (HSO4)4

(d) Pb3 (PO4)4

(e) (NH4)3 PO4

Out of the 5 compounds, which formula represents the

greatest total number of atoms?

Left side!!!

Number BQ and write it out Answer it (in another color/highlight it based

on what you read from my notes or textbook)

RIGHT side - End of notes

READ Ch 5.4 (pg. 133-135) first then take

notes

An empirical formula (e.f.) gives the relative number of atoms of each element in a compound.

A molecular formula (m.f.)gives the actual number of atoms of each element in a molecule of the compound.

For example, the m.f. for hydrogen peroxide is H2O2, and its e.f. is HO.

The molecular formula is always a whole number multiple of the empirical formula.

Left side!!!

Lets start a little review for the final exam

Draw the Matter Chart! (see next slide)

Pure substances may be either elements or compounds.

Elements may be either atomic or molecular.

Compounds may be either molecular or ionic.

Left side!!!

Atomic elements are those that exist in nature. ◦ basic units = atoms.

◦ Most of PT (~99%) elements fall into this category.

Molecular elements do not normally exist in nature(unstable as single atoms). Diatomic molecules —two atoms of that element bonded together. ◦ Basic units = molecules (unstable as single atoms)

There are 7 diatomic molecules – Name them!!

Left side!!!

Molecular compounds are compounds formed from two or more nonmetals. basic units = molecules.

Ionic compounds are compounds formed from a metal and nonmetal contains a cation (+ ions) paired with a anion (- ions).

basic units = formula units.

a. Krypton

b. CoCl2

c. Nitrogen

d. SO2

e. KNO3

f. Au

g. Na2O

h. H2O

Left side!!!

READ Ch 5.5 (pg. 135-137) first then take notes

2 types of Compounds ionic bonds molecular bonds (ch 5.8) (M + NM) (NM + NM) (M + PA)

ionic bond – electrical attraction between ions (charged atoms: cations and anions); e- are taken by one atom and given to another atom (like a magnet).

Ionic Compounds – Also called “Salts”

****Ionic bonding – only 2 types (sometimes 3 - rare)

1 Metal (cation) + 1 Nonmetal (anion)

or

1 Metal (cation) + 1 Polyatomic (anion) (see handout)

(The charges are “hidden” to make a neutral compound.)

Metals LOSE electrons.

become + ions = CATION

Group 1: Lose 1 electron to form 1+ ions

H+ Li+ Na+ K+

Label this on your PT!

Group 2: Loses 2 electrons to form 2+ ions

Be2+ Mg2+ Ca2+ Sr2+ Ba2+


Group 13: Loses 3 electrons to form 3+ ions

B3+ Al3+ Ga3+


Group 14: Loses 4 Electrons C4+ Si4+ Ge4+ Sn4+ Pb4+


Nonmetals GAIN electrons from metals

become - ions = ANION

ending to name changes to -ide

Group 15: Gains 3 electrons to form 3- ions

N3-

P3-

As3-

Nitride

Phosphide

Arsenide


Group 16: Gains 2 electrons to form 2- ions

O2-

S2-

Se2-

Oxide

Sulfide

Selenide


Group 17: Gains 1 electron to form 1- ions

F1-

Cl1-

Br1- Fluoride

Chloride

Bromide

I1- Iodide


Group 18: Stable Noble gases do not form ions!


Predicting Charges on Ions KNOW THESE !!!!

+1 +2 +3 +4 -3 -2 -1 0

Cd+2


I’m

Positive!

A metal ion A metal atom A nonmetal atom A nonmetal ion

I’m

Negative

I’m

Positive!

A metal ion A nonmetal ion

I’m

Negative

…the transfer of electrons produces ions,

which means…..

Ionic bonding!!!

cations (+) – Metals lose e- anions (-) – Nonmetals gain e-

monatomic ions – one ion Examples: Na+ or O-2

polyatomic ions - ions formed from two or

more atoms bonded together Examples: NH4

+ or SO4-2

Binary Ionic Compound – 2 atoms (M+NM)

Step 1– Write cation (metal) then anion (nonmetal)

Step 2 – Check to see if charges equal zero!!!

Step 3 – Criss-Cross Method - “Cross the charges” using subscripts to balance charges if they don’t balance out.

◦Don’t write 1’s.

Ba +2

Cl -1 = BaCl2

Write the correct formula and name the compounds containing the following ions:

1. Na+, S2-

2. Al3+, Cl-

3. Mg2+, N3-

4. Al3+, S2-

5. Zn+2, I-1

6. Ca+2, O-2

Left side!!!

READ Ch 5.6-5.7 (pg. 137-142) first then take

notes

1st step in naming an ionic compound – be able

to identify it as one. (sometimes the hard part)

◦ Ionic Compound (I.C.)

Lose (+ ions) and gain (- ions) electrons

Cation (+ ions) then anion (- ions)

◦ 3 types

◦ M + NM = binary I.C. (2 elements)

◦ M + P.A. = ternary I.C. (more than 2 elements)

◦ P.A. + P.A. = ternary I.C.

TRICKS – Transition and Other Metal Ions KNOW THESE !!!!

+1 +2 +3 +4 -3 -2 -1 0

Cd+2

Binary compounds - contain only two different

elements.

Draw this with notes!!!

cations – name doesn’t change

Example: Ba+2 barium ion

anions – remove the ending and add –ide

Example: Cl-

is not chlorine…. chloride ion

Naming: Cation (1st) then anion (2nd )

BaCl2 is barium chloride

Element Anion Symbol Anion Name

Bromine Br -1 Bromide

Chlorine Cl -1 Chloride

Fluorine F -1 Fluoride

Hydrogen H -1 Hydride

Iodine I -1 Iodide

Nitrogen N -3 Nitride

Oxygen O -2 Oxide

Phosphorus P -3 Phosphide

Sulfur S -2 Sulfide

Left side!!!

______

BaI2

______

AlF3

______

CaSe

______

KBr

_____

MgS

Sodium chloride

______________

Sodium phosphide

______________

Magnesium nitride

____________

Sodium nitride

____________

Aluminum oxide

_____________

Practice Problem #1:

Left side!!

READ Ch 5.6-5.7 (pg. 137-142) first then take

notes

Elements that can have more than one possible

charge MUST have a Roman Numeral.

Roman Numeral = # charge ion.

1+ or 2+ 2+ or 3+

Cu+, Cu2+ Fe2+, Fe3+

copper(I) ion iron(II) ion

copper (II) ion iron(III) ion

Draw this with notes!!!

- use Roman numeral in cation name

PbCl2

Pb2+ is cation

PbCl2 = lead(II) chloride

Metals with multiple charges

Complete the names of the following binary

compounds with variable metal ions:

FeBr2 iron (_____) bromide

CuCl copper (_____) chloride

SnO2 ___( ) ______________

Fe2O3 ____( )_______________

Hg2S ____( )_______________

Left side!!!

Formula Cation Name FeCl3 (Fe3+) iron (III) chloride CuCl ______ _________________ ______ ______ tin (IV) fluoride PbCl2 ______ _________________ Fe2S3 (Fe3+) _________________ ______ ______ Copper(II)oxide ______ ______ Lead(II)fluoride CrO3 ______ _________________ Cr2O3 ______ _________________

Left side!!!

Does the compound have

more than 2 elements?

Is the metal a

transition metal or

under staircase?

Cation

+

anion (ide)

Cation – use

Roman

Numerals

Metal

(check if T.M. or if

under staircase =

need R.N.)

+

Polyatomic names

(-ate or -ite)

yes

no

no

yes

Left side!!!

It will save

you!!

Left side!!!

Some ionic compounds contain polyatomic ions

(ions that are themselves composed of a group of

atoms with an overall charge).

Many polyatomic ions are oxyanions, anions containing oxygen.

If there are two ions in the series, the one with more oxygen atoms is given the ending -ate and the one with fewer is given the ending -ite. (BOTH SAME CHARGE!!) NO3

− nitrate SO42− sulfate

NO2− nitrite SO3

2− sulfite

If there are more than two ions in the series, then

the prefixes hypo-, meaning “less than,” and per-,

meaning “more than,” are used.

ClO − hypochlorite BrO

− hypobromite IO − hypoiodite

ClO2− chlorite BrO2

− bromite IO2− iodite

ClO3− chlorate BrO3

− bromate IO3− iodate

ClO4− perchlorate BrO4

− perbromate IO4− periodate

Writing Formulas for Ionic Compounds

Step 1– write cation (metal) then polyatomic

Step 2 – Charges have to equal zero!!!

“Cross the charges” if they don’t balance out.

Step 3-- Use parentheses around polyatomic ion

Practice Problems: Write the formula for each ionic compound.

copper(II) bromide ____________________

aluminum nitrite _________________________

barium hydrogen carbonate ___________________________

Cu+2 Br -1 = CuBr2 …(don’t show 1’s)

Al+3 NO2 -1 = Al(NO2)3

Ba+2 HCO3-1 = Ba(HCO3)2

1. aluminum nitrate

2. copper(II) nitrate

3. Iron (III) hydroxide

4. Tin(IV) hydroxide

Left side!!!


Write the formula for the following compounds. Lithium chloride Aluminum sulfide Copper(II) oxide

f)

Iron(III) chloride i) Calcium bicarbonate l

Potassium nitrite Potassium perchlorate

Ammonium carbonates )Iron(II) phosphate w)

Left side

Underlined letter = starting element symbol of the polyatomic

# consonants = # of oxygen atoms

# vowels = # negative charge on the ion

Left side!!!

Nick the Camel ate a

Creamy Clam for

Supper in Phoenix.

Manly Brad had an

Itch and took Aspirin.

Left side!!! – use different colors

Nick

NO3 -1

Underlined letter = starting element symbol of the polyatomic

# consonants = # of oxygen atoms

# vowels = # negative charge on the ion

N

3 consonants = O3

1 vowel = -1

Left side!!!


NaHCO3 K2SO3 MgSO4 KCN Ca(OH)2

NH4NO3 Zn(NO3)2 Li3PO4

Name the following ionic compounds:

Left side!!!


CuHCO3 FeSO3 CuSO4 Cr(CN)3 Cr(PO4)2

Sn(OH)2 W(NO2)5 Ti(CO3)2 CoPO4 PbCl2

Name the following ionic compounds:

Left side!!!

Write the formula for the following compounds. a) Barium oxide b) Sodium bromide

c) Copper(I) oxide d) Iron(II) chloride

e) Potassium nitrite f) Calcium hydroxide

g) Silver nitrate h) Ammonium chloride

i) Lithium phosphate j) Sodium nitrite

k) Sodium bicarbonate l) Calcium Carbonate

m) Sodium sulfate n) Iron(III) hydroxide

o) Copper(II) hypochlorite p) Magnesium sulfite

Left side!!! Practice Problem #7:

Ionic Covalent (molecular)

Metals & Only nonmetals

Nonmetals

lose/gain e- share e-

Ch 5.8 Naming Molecular Compounds

Left side!!!

The first step in naming a molecular compound is identifying it as one.

Remember - all molecular compounds form from two nonmetals. (no metals)

Use PREFIXES - indicate the # atoms in the compound.

Draw this with notes

Prefixes in Molecular Compounds

Number of atoms

Prefix Number of atoms

Prefix

1 mono- 6 hexa-

2 di- 7 hepta-

3 tri- 8 octa-

4 tetra- 9 nona-

5 penta- 10 deca-

Left side!!!

Anyone want a cold glass of dihydrogen monoxide?

Write the formula for dihydrogen monoxide?

Formula Common Name Molecular compounds name

H20 Water Dihydrogen monoxide

NH3 Ammonia Nitrogen trihydride

1. If there is only one atom of the first element, the prefix mono- is NOT WRITTEN.

CO2 mono carbon di- ox -ide

The full name is carbon dioxide.

2. The compound N2O also called laughing gas,

is named according to the first element, nitrogen, with prefix di-, followed by the second element, prefixed by mono-, and the oxide.

dinitrogen monooxide (Wrong!!)

HOWEVER….

Since mono- ends with a vowel and oxide begins with a vowel, an o is dropped and the two are combined as monoxide. The entire name is dinitrogen monoxide.

3. (Rule only for oxygen) – drop one of the “o”

Do not follow this rule for other elements.

Examples:

triiodide or tetraarsenide

a. P2O5

b. SO2

c. IF7

Left side!!! Practice Problem #1:


Name the following molecules.

a. N2O5

b. CO

c. Cl4F7

d. SO3

Left side!!!


Write the formula for each molecule.

a. nitrogen monoxide

b. carbon tetrachloride

c. diphosphorus nonaoxide

Acids are MOLECULAR compounds (share e-) that form ions when dissolved in water.

Composed of hydrogen, written first in their formula, and one or more nonmetals, written second.

Categorize acids into two groups: binary acids & oxyacids.

Make flowchart for the notes!!!

H and 1 nonmetal H and polyatomic


Binary acids are composed of hydrogen and a nonmetal. The names for binary acids have the following form:


HCl(aq) is hydrochloric acid.

HBr(aq) is hydrobromic acid.

HCl(g) refers to hydrogen chloride molecules in the gas phase, and not to the acid.

Give the name of H2S(aq) and H3P.

(Be careful of spelling)

2. Naming Oxyacids


Oxyacids are acids that contain oxyanions (polyatomic with oxygen)

The number of H+ ions depends on the charge of the oxyanion, so that the formula is always charge-neutral (criss-cross).

2. If the acid’s name ends with “______” without the “hydro-” prefix, the name of the anion used ends in “_______”. Therefore, it is an ____ acid.

Examples: perchloric acid = __________

acetic acid = ___________

3. If the acid’s name ends with “______”, the name of the anion used ends in “_______”. (It’s is also an oxy-acid.)

Examples: hypochlorous acid = __________

nitrous acid = ____________

sulfurous acid = ____________

-ic -ate

oxy-

-ous -ite

Left side

Naming Oxy-Acids

1. If the name of “(X)” ends in –ate… ____________-ic acid

2. If the name of “(X) ends in –ite… ____________-ous acid

Practice Problems: Name these acids.

H2SO4 H3PO3 HNO3 H2CO3 HC2H3O2 HClO2

Naming Binary Acids – 2 elements

If the name of “(X)” ends in –ide… hydro-__________-ic acid

Practice Problems: Name these acids.

H2S HCl HF

Left side

READ Ch 5.10 (pg. 146-148) first then take

notes

Left side

Start of 2nd Sem

right side notes only title and highlight - chemistry ch 5.1-5.3 title and highlight draw any...

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