South Garland High School Chemistry

Mr. Doolan

Unit 1 – Properties/Changes and Nomenclature

What is Chemistry?

- Chemistry is the study of matter, energy and the changes that occur between them

o we will learn how to properly describe matter

o we will look at many different types of changes and be able to properly

describe those changes

o we will work to quantify the energy associated with changes

o We will learn how to manipulate those changes to “coerce” them to do

what we want

o We will begin to understand how Chemistry shapes our everyday lives

What is Matter?

Matter is anything that has mass, takes up space and exhibits inertia

o Matter is composed of atoms (a little over 100 of them)

Ca2+

Na1+

There are three major classifications of elements in the periodic table:

Metals – generally have high electrical conductivity, high thermal conductivity, typically they are malleable

and ductile, lustrous. They also tend to lose electrons and form positive ions

Nonmetals – They are generally poor conductors of heat and electricity. Solid nonmetals are generally

brittle, with little or no metallic luster. Most nonmetals will gain electrons to form negative ions

Metalloids – these elements can have both properties of a metal and/or nonmetal depending on the

conditions and there is some dispute as to which elements are metalloids. The most commonly agreed upon

are: boron, silicon, germanium, arsenic, antimony and tellurium.

Basic arrangement of the periodic table:

Groups – are vertical columns

Elements within the same group have similar chemical properties

Elements in the same group have the same number of valence electrons

Periods – are horizontal rows

Periods are related to the energy levels of the atoms

****** The further the energy level is from the nucleus, the higher the energy associated with that energy ******

****** Electrons found in the outermost energy levels, called valence electrons, generally determine reactivity ******

H Li Na

N3-

Cl-

So if valence electrons determine chemical properties…

And each element in a group has similar chemical properties…..

Do all members of a group have the same number of valence electrons?

YES!!!!

Example 1: Put the following elements into categories that you would expect to have similar chemical properties:

Sodium, Magnesium, Aluminum, Potassium, Calcium

Example 2: The following elements: Calcium, Strontium, and Barium are all known to react with oxygen. Predict which

element will have the most energetic reaction. Justify your claim.

Properties and Changes:

Now that we have a basic understanding of the elemental chemical properties, lets go ahead and discuss properties

in general.

- There are 3 different types of properties we are going to be concerned with:

1. Chemical properties – are descriptions of the chemical reactivity of a substance. Basically it

tells us how something “could” react.

2. Extensive properties – are additive and the property is proportional to the amount of

material in the system. For example, both the mass and the volume of a diamond are directly

proportional to the amount that is left after cutting it from the raw mineral. Mass, volume,

length, and the amount of heat that can be absorbed are common extensive properties

3. Intensive properties - it is a physical property of a system that does not depend on the

system size or the amount of material in the system. Examples of intensive properties include

temperature, color, density, boiling point, melting point. No matter how small a diamond is

cut, it maintains its intrinsic hardness.

The ratio of two extensive properties is scale-invariant, and is therefore when 2 extensive properties are seen as a ratio

they become an intensive property. For example, the ratio of the extensive properties mass and volume (which is the

definition of density) is an intensive property.

Example 3: We are going to perform an experiment and need sodium. Off we go to the stockroom to get our sodium

compound and find that we are out…… Instead of going crazy, screaming, yelling and getting belligerent we

remember something and decide to grab a potassium compound instead. What did we remember and justify why

this just might work.

Sodium will react explosively with water

Lead nitrate and potassium iodide when mixed form a yellow precipitate

Example 4: Identify the properties listed below as either a chemical property, intensive property, or an

extensive property:

1.) The boiling point of water is 100oC 4.) Sodium metal is soft and malleable

2.) The density of the wood is 0.8 g mL-1 5.) Hydrogen gas is flammable

3.) 500mL of water takes 10 minutes to boil 6.) The mass of 95 mL of water is 95 grams

Going back to chemical properties…

What do we call it if a “described” reaction actually happens?

If a reaction actually happens we are going to call it a chemical change

Get it?

In a reaction, one chemical changes into another so it

should make sense that a chemical change occurs!

It is safe to say that whenever a chemical reaction occurs a chemical change has also

occurred! If we learn to spot chemical reactions, spotting chemical changes becomes

easier!

Some common signs that a chemical reaction is occurring:

1.) Formation of a precipitate

2.) Color change

3.) Release of energy (light and/or heat)

4.) Release of a gas (often seen as bubbles)

5.) ….

Example 5: Identify the properties listed below as either a chemical property or a physical property:

1.) Sodium metal is silver in color 4.) Sodium metal is soft and malleable

2.) Ammonium nitrate is a strong oxidizer 5.) Cesium reacts violently with water

3.) 500mL of water takes 10 minutes to boil 6.) The mass of 95 mL of water is 95 grams

Maybe by now you are asking if we can change substances WITHOUT changing the chemical make-up?

YES!!!!! Some common examples would be:

1) Bending something

2) Breaking something

3) Dissolving

4) Boil it

5) Melt it

6) …

Classification of Matter

States of Matter (mostly a vocabulary lesson)

solid – rigid; definite shape and volume; molecules close together vibrating about fixed points

virtually incompressible

liquid – definite volume but takes on the shape of the container; molecules still vibrate but also

have rotational and translational motion and can slide past one another BUT are still close

together slightly compressible

gas – no definite volume and takes on the shape of the container; molecules vibrate, rotate and

translate and are independent of each other VERY far apart highly compressible

- vapor – the gas phase of a substance that is normally a solid or liquid at room temperature - fluid – that which can flow; gases and liquids

Example 6: Distinguish between the following as either chemical changes or physical changes:

4.) Sodium chloride is dissolved in water 4.) Your bike rusts

5.) combustion of gasoline in your car engine 5.) Cooking an egg

6.) Milk souring 6.) Water boiling

Mixtures – can be physically separated. There are two types of mixtures:

homogeneous – have visibly indistinguishable parts so it all looks the same

heterogeneous – have visibly distinguishable parts, so you can easily see differences

means of physical separation include: filtering, fractional crystallization,

distillation, chromatography

Pure substances – compounds like water, carbon dioxide etc. and elements. Compounds can be

separated into elements by chemical means

- electrolysis is a common chemical method for separating compounds

into elements

- elements can be broken down into atoms which can be further broken down into - nuclei and electrons

- p+, n

0 and e

-

- quarks

Example 7: Classify the following as either element, compound, homogeneous mixture, heterogeneous mixture:

1.) Sodium Chloride

2.) Salt Water

3.) Sugar

4.) Iron

5.) Cookie Dough

6.) Air

7.) Helium

8.) Soil

9.) Water

10.) Arsenic

11.) Chunky Peanut Butter

Nomenclature – Naming Ionic compounds, Covalent compounds, and Acids

BINARY IONIC COMPOUNDS

Naming (+) ions: usually metals

monatomic, metal, cation simply the name of the metal from which it is derived. Al3+

is the

aluminum ion; transition metals form more than one ion; Roman Numerals (in) follow the ion’s name,

they are your friend—they tell you which charge is on that particular ion Cu2+

is copper(II);

(Yeah, the no space thing between the ion’s name and (Roman Numeral) looks strange, but it is the

correct way to do it. It’s called the Stock system developed by the German chemist Alfred Stock and

first published in 1916.)

NH4+

is ammonium

NO ROMAN NUMERAL IS USED WITH silver, cadmium and zinc. Why not? They only make one

valence state.

[Arrange their SYMBOLS in alphabetical order—first one is 1+ and the other two are 2+]

Naming () ions: monatomic and polyatomic

MONATOMIC--add the suffix -ide to the stem of the nonmetal’s name. Halogens are called the halides.

POLYATOMIC--quite common; oxyanions are the PA’s containing oxygen (Go, figure!)

- hypo--”ate” the least oxygen

- -ite--”ate” 1 more oxygen than hypo-

- -ate--”ate” 1 more oxygen than -ite

- hyper---ate--”ate” the most oxygen (often the “hy” is left off to read simply “per”)

Example: hypochlorite ClO

Chlorite ClO2

Chlorate ClO3

Hyper or more commonly Perchlorate ClO4

You can substitute any halogen in for the Cl.

Example 8: You have a yellow substance in a beaker. After heating, the substance has turned black and released a

very strong odor. As completely as you can, classify substance and justify your answer.

NAMING IONIC COMPOUNDS: The + ion name is given first followed by the name of the negative ion.

Example 9: Naming Type I Binary compounds

Name the following compounds:

a.) CsF b.) AlCl3 c.) CaCl2 d.) LiH

Example 10: Naming Type II Binary Compounds

Name the following compounds:

a.) CuCl b.) HgO c.) Fe2O3 d.) MnO2 e.) PbCl2

TYPE II:

Involve a transition metal that needs a

Roman numeral

Mercury (I) is Hg2+2

Exceptions: these never need a Roman

numeral even though transition metals.

Give up and MEMORIZE:

Ag+, Cd

2+, Zn

2+

(“Heavy Metal Bad Guys”)

Example 11: Name the following compounds:

a.) CoBr b.) MgCl2 c.) Al2O3 d.) CrCl3

Example 12: Name the following compounds with polyatomics:

a.) Na2SO4 g.) KBrO3

b.) Fe(NO3)3 h.) Na2SeO4

c.) Mn(OH)2 i.) NaOCl

d.) Na2SO3

e.) K2CO3

f.) CsClO4

Naming Binary Covalent Compounds (metals not present!!!!!)

USE PREFIXES!!!!!!!!

Anion will still have –ide ending

Prefixes will be based on subscripts of

elements 99% of the time

o The only exception to this is we never

put mono- in front of the cation

Naming Acids

ACIDS

Naming acids is actually easy. The nomenclature follows quite an elegant pattern:

Hydrogen, if present, is listed first followed by a suffix and finally the word “acid”.

If the negative ion’s name ends in:

-ide hydro[negative ion root]ic acid Ex: hydrosulfuric acid, H2S

-ate -ic acid Ex: sulfuric acid, H2SO4

-ite -ous acid Ex: chlorous acid, H2SO3

Example 13: Name each of the following compounds:

a.) PCl5 d.) SO3

b.) PCl3 e.) SO2

c.) SF6 f.) CO2

Example 14: Naming Acids

Name the following acids

a. HBr

b. H3PO4

c. H3PO3

d. H2CO3

e. H2CO2

f. HCl

g. HNO3

Example 15:

Name the following Compounds

a.) P4O10

b.) Nb2O5

c.) Li2O

d.) Ti(NO3)4

Writing Compound Formulas from Names

I do not want you to overthink this….. Essentially we are undoing what we have just done!

For the visual learners among you, here’s a “Cheat Sheet”. Practice, practice, practice!

Example 16:

Given the following names, write the formula for each compound:

a.) Vandium(V) Fluoride

b.) Dioxygen difluoride

c.) Rubidium oxide

d.) Gallium oxide

e.) Iron(III) phosphate

f.) Calcium nitrite

g.) Copper(II) Sulfate