Advanced Chemistry Unit #1 Review of Chemistry I. Material Unit conversions, Periodic Table review,...

Advanced ChemistryAdvanced ChemistryUnit #1

Review of Chemistry I. Material

Unit conversions, Periodic Table review, Polyatomic ion names, Nomenclature (ionic

& covalent), Stoicheometry (formula & equation), and “DIMO” (Mass / Mole

calculations)

Unit #1

Review of Chemistry I. Material

Unit conversions, Periodic Table review, Polyatomic ion names, Nomenclature (ionic

& covalent), Stoicheometry (formula & equation), and “DIMO” (Mass / Mole

calculations)

“SI Base Units” “SI Base Units”

SI - SI -

Revised version of the metric

system. Made up of seven base

units from which all others are

derived.

Revised version of the metric

system. Made up of seven base

units from which all others are

derived.

International system of units –

7 Base Units -7 Base Units -

Length -Length - meter m

Mass - Kilogram Kg

Time - second s (lower case)

Electric current - Ampere A

Temperature - Kelvin K

7 Base Units (con’t)-7 Base Units (con’t)-

Amount of substance -Amount of substance - mole mol (lower case)

Luminous intensity - Candela cd

Derived Units -Derived Units -

Volume -Volume - Cubic meter m3

Liter L

(L x w x h)

1 m3 = L?1 = mL?1000 = cm3?1000

Derived units (con’t) -Derived units (con’t) -

Density -Density - grams / cubic centimeter g/cm3

grams / milliliter g/mL

Density is symbolized by the Greek letter (rho) .

The formula is derived by dividing mass / volume.

Pressure -Pressure - Pascal Pa

Atmosphere Atm

Millimeters of Mercury mm Hg

101.325 Pa =1 atm =1 Bar =760 mm Hg =14.7 psi

Area -Area - Square meter m2

(l x w)

The “Conversion Line”- The “Conversion Line”-

A method to help with conversion of one metric unit to another.

Base unitm, g, L, …

K H Da d c m n p

To use the above: start with the unit you know, determine how many "places" you must move to get the unit you desire, then move your decimal in that direction, that many places.

K H Da d c m n p

Example 1: 20.0 mm = ? Km0.000020

K H Da d c m n p

Example 2: 123.0 L = ? mL123000.

K H Da d c m n p

Example 3: 0.454 g = ? mg454.

Temperature Relationships and Conversions

Kelvin (always capitalized)Kelvin (always capitalized)

Celsius

Boiling of H2O

Freezing of H2O

Absolute Zero

0 -273.15

273.15

373.15

K = C + 273.15

Solve for Celsius.

C = K - 273.15

Dimensional Analysis- Dimensional Analysis-

A technique used to convert and

combine numbers with like and different

units. This method is especially useful to

solve "story" problems like the ones we

will frequently see in Chemistry.

A technique used to convert and

combine numbers with like and different

units. This method is especially useful to

solve "story" problems like the ones we

will frequently see in Chemistry.

This technique simply requires you to "set up" and then "multiply and convert" fractions with the units that you are working.

Conversion Factor- Conversion Factor-

A ratio, including the units, set up

as a fraction and used to solve

"Chemistry problems.

A ratio, including the units, set up

as a fraction and used to solve

"Chemistry problems.

Example 1:Example 1:

1500 mL = ? L1500 mL = ? L

To solve set up as follows:

1500 mL x 1 L 1000 mL

= 1.5 L

How long is a 1,000,000 seconds (in days)?

1,000,000 = 11.57 days

According to the National Debt

Clock, the national debt is (visit web site:

nationaldebtclock.com) "X" trillion of dollars.

How long until 1 trillion seconds pass?

1,000,000,000,000 sec = ?

A few periodic short cuts.A few periodic short cuts.

Series / Period Series / Period

horizontal rows on the periodic chart.

All elements in the same series or period are in the same energy level.

Family / Group Family / Group

vertical columns on the periodic chart

All elements in the same family or group have the same number of valence electrons.

Metals- Metals- Elements that are usually solid /

liquid at room temperature, good conductors of heat and electricity, malleable, ductile, often shiny (luster).

Elements that are usually solid / liquid at room temperature, good conductors of heat and electricity, malleable, ductile, often shiny (luster).

Examples: Magnesium

Sodium

Non-metals - Non-metals -

Elements that may be either solid, liquid, or gaseous, poor conductors of heat and electricity, brittle, and often dull.

Elements that may be either solid, liquid, or gaseous, poor conductors of heat and electricity, brittle, and often dull.Examples: Argon

Sulfur

Iodine

Two specific types of non-metals are:Two specific types of non-metals are:

1) Metalloids

2) Gases

1) Metalloids

2) Gases

Metalloids- Metalloids-

Non-metals with some metal like

properties.

Often used in electronics.

Non-metals with some metal like

properties.

Often used in electronics.

Examples: Silicon

Arsenic

Gases - Gases -

Elements that are "gases". They

are matter with no definite shape or

volume, are fluid (they "flow").

Elements that are "gases". They

are matter with no definite shape or

volume, are fluid (they "flow").

Examples: Oxygen

Helium

Electronegativity - Electronegativity -

The measure of the attraction an atom has for shared electrons. (How much an atom wants electrons.)

Animation of Electronegativity

The "Ups and Downs" of ElectronegativityThe "Ups and Downs" of Electronegativity

Compare the electronegativities of the elements.Compare the electronegativities of the elements.

QuickTime™ and aTIFF (Uncompressed) decompressor

are needed to see this picture.

How to use electronegativity to predict the type of chemical bond

that will form:

that will form:1) Calculate the difference in electronegativity

between the two elements that are going to bond. 1) Calculate the difference in electronegativity

between the two elements that are going to bond.

These values are on the back of your periodic chart, as well as in various chemistry texts.

that will form:

The difference is determined by subtracting the smaller number from the larger.

The element with the larger electronegativity will tend to have possession of (“hog”) the shared electrons more than the other element.

that will form:

If the difference is 1.6 or greater; the bond will be ionic.

Example: NaClExample: NaCl

Na= 0.93

2.23 = Ionic Bond

that will form:

If the difference is less than 1.6, and 0.4 or greater; the bond will be polar covalent.

Example: CO2Example: CO2

C=2.55

0.89 = Polar Covalent Bond

that will form:

If the difference is less than 0.4; the bond will be non-polar covalent.

Example: Cl2Example: Cl2

0.00 = Non-Polar Covalent Bond

Remember: Remember:

Ion- Ion- an atom or group of atoms that has either lost or gained electron(s) and as a result has an electric charge.

Cation- is a positively charged ion.

Anion- is a negatively charged ion.

Cation-

A positively charged ion.

A former student once remembered this by noticing that if you add a "u", it spells caution (Caution). And, you should exercise caution around positively charged wires.

Anion-

A negatively charged ion.

Remember: an Anion is A (A) / n (negative) / ion (ion)

Consider this:

If all atoms have negatively charged electrons, shouldn't every sample of matter have a negative charge?

Why not?

Because positively charged protons off set the negative charge of the electrons. And, unless it is an ion, it has the same number of protons as electrons.

Polyatomic ion namesPolyatomic ion names

Polyatomic ion -Polyatomic ion -An ion composed of 2 or more atoms. The

charge is assumed to be on the entire molecule.

Example: CO3-2 (Carbonate)

The charge is dispersed over the entire molecule.

Remember these must be memorized. Use the flash cards that you were given.

Nomenclature -Nomenclature -

The naming of chemical compounds.

There are three different sets of rules used to name simple inorganic compounds.

Ionic Nomenclature:Ionic Nomenclature:

The type of ionic compound will determine which set of rules to use.

There are two general types of ionic compounds:

Those in which the cation has only one possible charge.

Examples:Examples:

Na, Ca, Mg, Al, Ba

Those in which the cation has more than one possible charge.

Examples:Examples:

Fe, Cr, Cu, Mo, the transition elements.

If the cation has only one possible charge, name as follows:

Cation:Cation: Simply use the entire name of the element. (It will be capitalized).

Anion:

Use the entire name of the element; minus the ending, plus the suffix "-ide". (It will be lower case).

If Polyatomic Cation or Anion:If Polyatomic Cation or Anion:

Use the whole name of the Polyatomic ion. Regardless if cation or anion.

Examples:Examples:

Lithium chlorideLithium chlorideLiCl

MgS Magnesium sulfide

BeCl2 Beryllium chloride

KNO3 Potassium nitrate

(NH4)2SO4 Ammonium sulfate

Name this compound:Name this compound:

FeOFeO

If the cation has more than one possible charge, name as follows:

Simply use the entire name of the element, followed by a roman numeral (in parenthesis) that indicates the charge of the cation. (It will be capitalized).

Cation:

Anion: Same as the all other ionic compounds.

Polyatomic: Same as other ionic compounds.

Examples:

TiO2 Titanium (IV) oxide

Pb(OH)4 Lead (IV) hydroxide

FeSO4 Iron (II) sulfate

FeO Iron (II) oxide

Fe2O3 Iron (III) oxide

Covalent Nomenclature:Covalent Nomenclature:

Usually, the least electronegative element is written first.

Examples: CO2, N2O, SO3

Covalent Nomenclature:Covalent Nomenclature:

Prefixes are used to indicate the number of each atom present in the compound.

1 atom = Mono (except when referring to the first element; in this case you will not use a prefix.)

Covalent Nomenclature:Covalent Nomenclature: 2 atoms =

3 atoms =

4 atoms =

5 atoms = 6 atoms =

7 atoms =

8 atoms =

9 atoms =

10 atoms =

The first element will be named by using the prefix (indicating the number of atoms) + the elements name.

Example: N2O4 = Dinitrogen

NOTE: DO NOT USE “MONO-” ON THE FIRST ELEMENT !

The second element will be named by using the prefix (indicating the number of atoms) + the element’s name, minus the ending, plus “-ide”.

Example: N2O4 = Dinitrogentetroxide

Binary acid Nomenclature -Binary acid Nomenclature -

Binary acid -Binary acid - An acid composed of only two elements: Hydrogen and usually a halogen.

Named:

Hydro +Halogen name, - ending, + “_ic acid”

Example:Hydrochloric acid, Hydrofluoric acid

Ternary acid Nomenclature -Ternary acid Nomenclature -

Ternary acid -Ternary acid - An acid composed of only three elements: Hydrogen and a polyatomic ion.Named:

Name of Polyatomic ion, “- ate”ending, + “_ic acid”

Example:Carbonic acid, Nitric acid

StoicheometryStoicheometry

Balancing the charges on ions that are forming a molecule so that they add up to zero.

Balancing chemical equation so the number of particles of reactants is equal to the number of particles of products.

The total electrons gained must equal the number lost.

4 Steps to "balancing" an ionic compound:

Step 1:Step 1:

Write the cation and the anion next to each other, leave some space between them.

Step 2:Step 2:

Write the absolute value of the cation's charge as the subscript to the anion. (If this value is "1", you don't have to write anything.)

Step 3:Step 3:

Write the absolute value of the anion's charge as the subscript to the cation. (If this value is "1", you don't have to write anything.)

Step 4:Step 4:

Write the above determined subscripts in lowest terms.

Write the balanced formulaformed by combining the followingions: K & P

Example 1:

Write the balanced formulaformed by combining the followingions: Al & O

Example 2:

Write the balanced formulaformed by combining the followingions: Mo (VI) & O

Example 3:

Sometimes, you may have a

formula and you will need to determine the

charge on the cation (this occurs when

naming transition element compounds).

Use the following steps to achieve this

Transition element Transition element

Elements that have "d"

and "f" sub-levels. (See unit #3 if

necessary to review "d & f

sublevels").

Elements that have "d"

and "f" sub-levels. (See unit #3 if

necessary to review "d & f

sublevels").

Transition Element Stoicheometry:

Step 1:Step 1:

Write the formula, and separate the cation and anion with a cross.

Step 2:Step 2:

Multiply the charge of the anion with the subscript of the anion (this will always be a negative number); and write this number in the lower right corner of the cross.

Step 3:Step 3: Write the absolute value of the number calculated above (in step 2) in the lower left corner of the cross.

Step 4:Step 4: Divide the number calculated in step 3 above by the subscript of the cation. This calculated value is the charge of the cation.

Example 1:Example 1: WS2

Example 2:Example 2: CrO3

Example 3:Example 3: MoO

Example 4:Example 4: MnO2

Balancing Chemical EquationsBalancing Chemical Equations

In all balanced equations:In all balanced equations:

# of atoms of each element on the left of the "yields" arrow,

# of atoms of each element on the right of the "yields" arrow

must equal

Many equations can be

balanced by trial and error…

However, the following five rules will

make balancing quicker.

1. Write the correct formulas:1. Write the correct formulas:

a) For all reactants to the left of the arrow.

b) For all products to the right of the arrow.

c) If more than one reactant or product, separate them with a "plus" sign.

2. Once the correct formula is written: NEVER

change the subscript(s).

2. Once the correct formula is written: NEVER

change the subscript(s).

3. Set up a chart:3. Set up a chart:

a) with all atom types down the left side

b) 2 columns:

i) one labeled left

ii) the other labeled right

4. Start with any elementthat appears only once

on both sides of the equation.

4. Start with any elementthat appears only once

on both sides of the equation.

5. Balance the elements oneat a time by adding

coefficients in front of the formulas.

5. Balance the elements oneat a time by adding

coefficients in front of the formulas.

a) Remember: no coefficient = 1.

b) Multiply coefficients by the subscript to determine the number of atoms.

c) Adjust coefficients as necessary.

What thing can we determine from a balanced equation?

1. Proportions of reactants & products(Remember: the coefficient shows

mole ratio.2. # of atoms / molecules / formula units /

3. From the mole ratio… we can use DIMO tocalculate grams.

Hydrogen and Iodine react to form Hydrogen iodide.Hydrogen and Iodine react to form Hydrogen iodide.

H2 + I2 →→→ HIH2 + I2 →→→ HIH2 + I2 →→→ 2HI

Hydrogen bromide and Oxygen react to form water and BromineHydrogen bromide and Oxygen react to form water and Bromine

HBr + O2 →→→ H2O + Br24HBr + O2 →→→ 2H2O + 2Br2

Carbon dioxide and water in the presence of sunlight and chlorophyll react to produce glucose (C6H12O6) and oxygen.

6CO2 + 6H2O →→→ C6H12O6 + 6O26CO2 + 6H2O →→→ C6H12O6 + 6O2CO2 + H2O →→→ C6H12O6 + O2

Copper and concentrated Nitric acid react to form Copper (II) nitrate, water, and Nitrogen dioxide.

Cu + 4HNO3 → Cu(NO3)2 +2H2O + 2NO2Cu + 4HNO3 → Cu(NO3)2 +2H2O + 2NO2Cu + HNO3 →→→ Cu(NO3)2 + H2O + NO2

Sodium hydroxide and Sulfuric acid react to yield Sodium sulfate and water.

2NaOH + H2SO4 →→→ Na2SO4 + 2H2O2NaOH + H2SO4 →→→ Na2SO4 + 2H2ONaOH + H2SO4 →→→ Na2SO4 + H2O

Barium hydroxide and Nitric acid react to form Barium nitrate and water.

Ba(OH)2 + 2HNO3 →→→ Ba(NO3)2 + 2H2OBa(OH)2 + 2HNO3 →→→ Ba(NO3)2 + 2H2OBa(OH)2 + HNO3 →→→ Ba(NO3)2 + H2O

DIMO - DIMO -

An acronym that means:

Divide In Multiply Out.

An acronym that means:

Divide In Multiply Out.

It is a drawing that you have to be able to reproduce and use.

# of moles

# of grams # of particles

# of liters of a gas

Chart mass Avagadro’s #

4 Steps to use the DIMO chart.4 Steps to use the DIMO chart.

1 ) Determine the chart mass of thesubstance you're working with.

2) Deal with the concentration of that substance.

3) Deal with the volume of the solution you're working with.

4) Use "DIMO" to solve.

How many grams of NaOH are in 1 liter of a 1M solution of the NaOH?

Example 1:

STEP 1: Determine the chart mass

Example 1 (con’t.):

STEP 1: 40 g/mol

STEP 2: Deal with the concentration

STEP 1: 40 g/mol

STEP 2: 1 mol/L

STEP 3: Deal with the volume

STEP 1: 40 g/mol

STEP 2: 1 mol/L

STEP 3: 1 mol of NaOH in sample

STEP 4: Use "DIMO" to solve

How many grams of NaOH are in 1 liter of a 1M solution of the NaOH?

Solution to Example 1:

There are 40 g of NaOH in 1 liter of a 1M solution of NaOH.

0.75 liters of a 0.5M solution contains how many grams of CaCl2?

Example 2:

STEP 1: 111 g/mol

STEP 2: 0.5 mol/L

STEP 1: 111 g/mol

STEP 2: 0.5 mol/L

STEP 3:0.375 mol of CaCl2 in sample

How many grams of CaCl2 are in 0.75 liter of a 0.5M solution of the CaCl2?

There are 41.625 g of CaCl2 in 0.75 liter of a 0.5M solution of CaCl2.

Notice in the previous examples we calculated the number of grams of a substance.

In the next example, we will determine how many moles of a substance are in a given volume of a solution.

Notice in the previous examples we calculated the number of grams of a substance.

In the next example, we will determine how many moles of a substance are in a given volume of a solution.

What is the Molarity of a solution created by dissolving 150 grams of NaI into 250 mL of distilled water?

Example 3:

STEP 1: 150 g/mol

STEP 2: 150 g / 0.25 L

STEP 1: 150 g/mol

STEP 2: 150 g / 0.25 L

STEP 3: 600 g / 1 L

What is the Molarity of a solution created by dissolving 150 grams of NaI into 250 mL of distilled water?

There are 4 moles of NaI in 1 liter of the solution of NaI.

Therefore the molarity is ____4M

600 g of NaI is 4 moles

Finding the number of particles (atoms or

molecules) is done the same way: except you

would divide or multiply in or out by "Avagadro's

number".

You will get practice doing this on your study

guide.

Finding the number of particles (atoms or

molecules) is done the same way: except you

would divide or multiply in or out by "Avagadro's

number".

You will get practice doing this on your study

guide.

Advanced Chemistry Unit #1 Review of Chemistry I. Material Unit conversions, Periodic Table review,...

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