science 10 chemistry notes what is chemistry?

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1 Science 10 – Chemistry Notes Name: _________________ What is Chemistry? Chemistry is the science in which substances are examined to find out: - What things are made of - How they act under different conditions - How they are combined or separated to form other substances. Essentially, chemistry is the study of ____________________. Matter: - anything that has __________________ and takes up __________________. - Is the make up of the entire universe. - Is made up of atoms and elements. Periodic Table of the Elements Metals: Found to the _____________ of the “ladder”. Generally shiny ______________ at room temperature and _______________ conductors of heat and electricity. Non-Metals: Found to the ____________ of the “ladder”. Exist in all three states of matter, ___________, and ____________ conductors. Metalloids: Found along ______________________ of the ladder. Have properties of ___________ metals and non-metals. Horizontal rows are called ______________________. Vertical columns are called _______________ or ________________. Periodic Table Analogy Lab How to Read the Periodic Table:

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Page 1: Science 10 Chemistry Notes What is Chemistry?

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Science 10 – Chemistry Notes Name: _________________

What is Chemistry? Chemistry is the science in which substances are examined to find out:

- What things are made of

- How they act under different conditions

- How they are combined or separated to form other substances.

Essentially, chemistry is the study of ____________________.

Matter:

- anything that has __________________ and takes up __________________.

- Is the make up of the entire universe.

- Is made up of atoms and elements.

Periodic Table of the Elements

Metals: Found to the _____________ of the “ladder”.

Generally shiny ______________ at room temperature and

_______________ conductors of heat and electricity.

Non-Metals: Found to the ____________ of the

“ladder”. Exist in all three states of matter,

___________, and ____________ conductors.

Metalloids: Found along ______________________ of

the ladder. Have properties of ___________ metals and

non-metals.

Horizontal rows are called ______________________.

Vertical columns are called _______________ or

________________.

Periodic Table Analogy Lab

How to Read the Periodic Table:

Page 2: Science 10 Chemistry Notes What is Chemistry?

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Anatomy of an Atom Element: A _____________ substance that ______________ be broken down

into a simpler substance (made up of ____________________ kind of atom).

Atom: the basic unit of an ______________________.

Let’s determine which element this is:

How many electrons?

_____________________

How many valence electrons? ______________

How many protons? ______________________

How many neutrons? _____________________

Atomic number = number of protons = __________

Atomic mass = # protons + # neutrons = ______________

Element Symbol Atomic

#

Atomic

Mass

Protons

p+

Neutrons

n0

Electrons

e-

Cesium

Selenium

Bromine

Assignment: How to Count Protons, Neutrons and Electrons

Bohr Diagrams of Atoms Neils Bohr developed a theory to identify where ____________________ are found

around the nucleus (Hotel Analogy)

e- surround the nucleus in _______________/ _____________/_________________

1st Ring can hold max ____ e- 2nd Ring can hold max _____e- 3rd Ring can hold max ______e-

Ex) Na atom (____________ e-) ex) Sulfur atom (____________ e-)

Page 3: Science 10 Chemistry Notes What is Chemistry?

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Assignment: Bohr Diagram Periodic Table Worksheet

How Atoms Become Stable (p+≠ e-)

Electrons in the outermost ring are called ____________________________

When outermost shell is full, element is ________________

Atoms may gain or lose ___________________________ in order to get a full valence shell,

thus becoming _______________ (charged particles).

Ex) Sodium atom Outer shell has ______ electron Sodium ION

P+ = e- = P+ = e- =

Ex) Fluorine atom Outer shell has ______ electron Fluoride ION

P+ = e- = P+ = e- =

Group Valence e- Lose or Gain

1 1 lose 1 gain 7

2 2 lose 2 gain 6

3/13 3 lose 3 gain 5

4/14 4 lose 4 gain 4

5/15 5 lose 5 gain 3

6/16 6 lose 6 gain 2

7/17 7 lose 7 gain 1

8/18 8 lose 8 gain 0

Page 4: Science 10 Chemistry Notes What is Chemistry?

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Fill in the chart for the following:

Atom Bohr diagram for

atom

Bohr diagram for

stable ion

Gained/lost

electrons

Formula of

ION that is

formed

Same number of

electrons as what

Noble Gas?

a) Lithium

lose ______

gain _____

b) Nitrogen

lose ______

gain _____

Assignment: Atom/Ion Worksheet

- Only _____________________________ can be gained or lost from an atom.

o The atomic number is different for every element on the periodic table of the

elements. It is characteristic for that element. You ______________________

change the number of protons! If you change the number of protons, you change the

atomic number, and you have a different element!!

- If an atom loses an electron, it becomes a positive ion (_____________________)

- If an atom gains an electron, it becomes a negative ion (____________________)

Determining p+, n0, e- of Ions

Ions ≠ Neutral # ______________ ≠ # ____________

Ex) Li1+ atomic # = p+= no = e- =

Ca2+ O2-

p+ 16 13

no

e- 18 10

Assignment: Determining Protons, Neutrons, and Electrons for Ions

Gold Penny Lab

In-Class Assignment: p+, n0, e- for atoms/ions; Bohr diagrams for atoms/ions,

gained/lost electrons, ion that’s formed, same Bohr diagram as what atom?

Page 5: Science 10 Chemistry Notes What is Chemistry?

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How Elements Form Compounds In order for atoms to have a stable valence shell, they will link up with other atoms by _______________, giving up

or __________________ electrons. This is how elements combine to form compounds.

There are two major types of compounds that can form between atoms:

1. Ionic Compounds: where _______________ bond with ________________.

2. Covalent Compounds: where _________________ bond with other __________________.

1. Ionic Compounds Ex) Sodium + Chlorine Here we see that sodium (______________) will give its

valence electron to chlorine (_________________) so that

they both have stable shells.

Once this happens, the ionic charge of sodium will be _____

and the ionic charge of chlorine will be ____.

These two opposing charges will attract each other and a

chemical bond will be formed creating the compound

__________________.

Sometimes, more than one electron can be transferred.

Ex) Magnesium + Oxygen

This compound’s name is __________________________.

Sometimes more than one atom of each element will have to be involved.

Ex) Beryllium + Fluorine

This compound’s name is ___________________________.

Assignment: Making Simple Ionic Compounds

Page 6: Science 10 Chemistry Notes What is Chemistry?

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2. Simple Ionic Compounds (M + NM)

a) Writing Formulas (Ions→ formula)

Writing Formulas for Ionic Compounds

Look up the Symbol and Charge

left-hand side right hand side

metal and non-metal (or polyatomic)

Figure out how many of each element you need to make sure your charges cancel out

THE CHARGES GO AWAY BECAUSE YOUR PLUSES CANCEL YOUR MINUSES!!!!

ionic formula ionic formula

left-hand side right hand side left-hand side right hand side

sodium phosphide magnesium sulfide

Na1+ P3- I need 3 Na1+ Mg2+ S2- I need 1 Mg2+

Na1+ to cancel out P3- to cancel out 1

Na1+ Na3P S2-

MgS

Given the name, write the formula

Potassium bromide____________________

Aluminum chloride___________________

Calcium phosphide ___________________

Lithium nitride_____________________

Potassium selenide ___________________

c) Naming Simple Ionic Compounds ( M + NM) Formula → Name ionic naming ionic naming

Na3P CaI2

left-hand side right hand side left-hand side right hand side

sodium phosphide calcium iodide

Ex) NaCl K2O CaF2

BaS2 Na3N Li3As

Assignment:

Naming Ionic

Compounds and

Writing Ionic

Formulas

Worksheet

Page 7: Science 10 Chemistry Notes What is Chemistry?

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3. Transition Metal Ionic Compounds (M + NM)

a) Writing Formulas (Name Formula)

Copper (II) sulfide _____________________

Copper (I) sulfide ____________________

iron (III) oxide _____________________

mercury (II) phosphide ___________________

b) Naming (Formula Name)

MnCl2 Cu3N2

left-hand side right hand side left-hand side right hand side

manganese (II)? chloride copper (I)? nitride

OR manganese (III)? chloride OR copper (II)? nitride

Mn? Cl1- 2 minuses Cu? N3-

Cl1- Cu? N3-

Cu?

therefore must be Mn+2 so 1 Mn cancels therefore must be Cu+2 so 3 Cu cancels

with 2 Cl1- with 2 N3- manganese (II) chloride copper (II) nitride

PbO ______________________________ PbO2 ______________________________

CoS _____________________________ Co2S3 _____________________________

Assignment: Ionic Compounds: Metals with More than one Charge

4. Polyatomic Compounds

a) Writing Formulas (Name Formula)

ionic formula ionic formula

left-hand side right hand side left-hand side right hand side

sodium iodate gold (III) nitrate

Na1+ IO3- I need 1 Na1+ Au3+ NO3 1- I need 1 Au3+

to cancel out 1 IO3- NO3 1- to cancel out 3

NaIO3 NO3 1- NO33-

Au(NO3)

Page 8: Science 10 Chemistry Notes What is Chemistry?

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sodium chlorite

barium nitrate

magnesium carbonate

calcium hydroxide

b) Naming (Formula Name)

Na3PO4 Ca(OH)2

left-hand side right hand side left-hand side right hand side

sodium phosphate calcium hydroxide

Name the following compounds:

Na2SO4 Al(ClO3)3 NH4NO3 Rb2HSO3

Assignment: Making Polyatomic Ionic Compounds Using Models Activity

Assignment: Polyatomic Compounds Names and Formulas Worksheet

Understanding Concepts

In your own words, explain what is meant by the term “polyatomic ion”. Give 2

examples.

1. Covalent (Molecular) Compounds (Non Metal/Non Metal)

Are formed when 2 NON-METALS bond Here, electrons are SHARED, not transferred as they are in ionic compounds.

Naming: A prefix is used to indicate the number of each element in the compound. (The exception is we don’t use

mono- for the first element). Charges are not of concern in covalent compounds.

Drop the ending of the second element and add –ide.

Examples: CCl4 carbon tetrachloride

N2O3 dinitrogen trioxide

Prefix Number

Mono- 1

Di- 2

Tri- 3

Tetra- 4

Penta- 5

Hexa- 6

Hepta- 7

Octa- 8

Nona- 9

Deca- 10

Page 9: Science 10 Chemistry Notes What is Chemistry?

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Practice: Name the following covalent compounds. 1. PBr3 ______________________________________________

2. P2O3 _______________________________________________

3. CF4 _______________________________________________

4. SO2 _______________________________________________

5. N2O ______________________________________________

Writing Formulas Completely ignore the charges of the non-metals!!! The prefixes will tell you how many atoms of each element you need.

DO NOT reduce compounds to lowest form! Leave them as the name states.

Examples: Nitrogen trihydride NH3

Dinitrogen tetraoxide N2O4

Practice: Write the formulas for the following covalent compounds.

1. tetraphosphorus triselenide _______________

2. disilicon hexabromide _______________

3. diarsenic trioxide _______________

4. selenium monosulfide _______________

5. carbon tetrabromide _______________

6. boron trifluoride _______________

Page 10: Science 10 Chemistry Notes What is Chemistry?

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Understanding Concepts

1. How can you tell the difference between an ionic compound and a molecular

compound?

2. What kinds of atoms form molecular compounds?

3. How do the atoms in molecular compounds form stable electron arrangements?

In other words, what happens to the electrons?

Assignment: Covalent (Molecular) Compounds: Names and Formula Worksheet

BONUS: Mixed Ionic and Covalent Compounds

IN-CLASS ASSIGNMENT #2: Naming and Writing Formulas for ionic, metals with more than one

charge, polyatomic ions, covalent, and mixed naming

2. Hydrocarbons: Alkanes and Alkenes

a) Alkanes An alkane is a saturated hydrocarbon. In other words, an alkane is a long chain of carbon linked

together by single bonds.

The general formula for alkanes is CnH2n+2.

Formula Structure

o The simplest alkane is methane

Formula Structure

o The next simplest is ethane

o The series continues indefinitely

**Each C must have 4 bonds **

Page 11: Science 10 Chemistry Notes What is Chemistry?

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Naming Alkanes Naming alkanes is quite simple: just use prefixes counting the number of carbon atoms in the

formula and add the suffix –ane.

The prefixes are as follows:

Examples:

NAME:

Alkanes can be symbolized in a few different ways:

Molecular Formula Expanded structural Formula Condensed structural Formula

Ex) propane

b) Alkenes Alkenes are unsaturated hydrocarbons which means their carbon structure contains double bonds.

The general formula for alkenes is CnH2n

The simplest alkene is ethene (C2H4)

Naming Alkenes Naming alkenes is generally the same as naming alkanes, but with the suffix -ene and a

number indicating which carbon the double-bonded is attached to in the chain.

You can number the carbons either left to right or right to left. You must pick whichever

way gives the carbon with the double bond the LOWEST possible number.

Ethene and propene do not require numbers, since there is no question as to where the

double-bonded carbon is in the structures.

Example: propene C3H6

Example: butene C4H8 can have the double bonded

carbon in two different places. NAME:

NAME:

**Give the double bond the lowest

number **

Page 12: Science 10 Chemistry Notes What is Chemistry?

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Assignment: Simple Alkanes and Alkenes

Naming Alcohols

Alcohols are organic carbons similar to alkanes but one of the hydrogen’s is substituted with a

hydroxide group, OH.

Alcohols are named by replacing the final –e of the alkane with the suffix “–ol”.

The location of the hydroxyl group is indicated with a number. The chain is numbered to give the

alcohol functional group the lowest possible number.

Example)

NAME:

Draw 2-pentanol and 3-pentanol

Assignment: Naming Alcohols

Practice Exam/Review

EXAM