Chemistry Sem 1 Exam Review

Chemistry Semester 1 Exam

Review for Exam

• ​Matching (atomic structure) 5 pts

• Properties & Change 2 x 2pts = 4 pts

• Atomic Structure 5 x 2 pt = 10 pts

• Per. Table Organization 5 x 2 pt = 10 pts

• Electrons in Atoms 2 x 3 pts = 6 pts

• Ionic Compounds 8 x 2 pts = 16 pts

• Covalent Compounds 4 x 2 pts = 8 pts

• Acids 4 x 2 pts = 8 pts

• Equations & Balancing 5 x 3 pts = 15 pts

• Types of Equations 4 x 2 pts = 8 pts

• Essay ( Atomic Structure/ eqns) 1 x 10 pts = 10 pts

• 45 questions 100 pts
  

Chemical/Physical Properties and Changes

Physical Properties

• Properties that can be observed without changing the identity of the substance.

Chemical Properties

Chemical properties describes how a substance reacts to other substances.

The question to ask!

Are these properties determined without changing the identity of the substance?

Multiple Choice

Water (H₂O) freezes at zero degrees celsius. Is freezing an example physical or chemical property?

• physical property

• chemical property

Multiple Choice

An iron nail is left outside on the porch exposed and rusts. Is rusting an example of a physical or chemical property?

• physical property

• chemical property

Multiple Choice

An object catches on fire. Is this flammability an example of physical or chemical property?

• physical property

• chemical property

Physical Changes

Physical changes have the same identity but change in physical state or appearance.

Can you get the original substance back?

Chemical Changes

Chemical changes involve how substances react to other substances.

Chemical changes create new substances. (Not just changes in appearance.)

Can you get the original substance back?

Multiple Choice

Is baking a cake a physical or chemical change?

• physical change

• chemical change

Multiple Choice

Is dissolving sugar into water a physical or chemical change?

• physical change

• chemical change

Multiple Choice

Is boiling water a physical or chemical change?

• physical change

• chemical change

Atomic History

What is Matter made of?

• Since ancient times, scientists have pondered this question.

• Democritus, a Greek philosopher around 400 BC, proposed matter was made of basic units that could not be cut apart.

• He called these atomon (Greek for "uncuttable").

A Differing View

• Aristotle disagreed with Democritus's idea.

• He argued that matter made of particles would fall apart, like sand.

• Aristotle proposed matter was infinitely divisible.

• He also proposed the idea of basic elements: fire, earth, air, water and aether (the stuff of the heavens)

So, who was right?

• Neither idea could be proven correct because there was no experimental support.

• So both ideas reigned for approx. 2,000 years...

Multiple Choice

Who proposed the idea of atoms?

• Democritus

• Aristotle

• Einstein

• Newton

Sir Joseph John Thomson

• 1897

• Worked with Cathode Ray Tubes (CRTs)

• Credited with discovering the electron

Electrons are matter

• A paddlewheel was placed in the CRT

• When the beam was turned on, the wheel moved down the CRT

• Energy, like light, would not make the wheel move.

• Thus, electrons have mass and are matter (not energy).

Thomson's Atomic Model

• The atom is neutral, so the atom is a big positive sphere with negative electrons throughout.

• Same in all directions

• Called the "Plum-Pudding" model because electrons are like raisins in a plum pudding.

Ernest Rutherford (1911 / England)

​Known For: Protons (positive charged) and atoms were mostly empty space

Experiment:
Gold Foil Experiment

Visual Representation

Atomic Structure

Multiple Choice

What is the charge of a proton?

• Negative

• Positive

• Neutral

Multiple Choice

What is the charge of a neutron?

• Negative

• Positive

• Neutral

Multiple Choice

1. 1) What is the charge of the nucleus of an atom?

• negative

• positive

• neutral

• none

Multiple Choice

Protons and neutrons are found inside nucleus

• True

• False

Multiple Choice

The positively charge (+) particles of an atom

• Proton

• Electron

• Neutron

Multiple Choice

The no charge (n0) particles of an atom.

• Proton

• Electron

• Neutron

Multiple Choice

The negatively charge (-) particle of an atom.

• proton

• electron

• neutron

​An ATOM is Neutral. That means it has no charge.

​So...It has to have the same number of electrons as it has protons!

​P +1

e -1

Net Charge is 0

Multiple Choice

Protons are DIFFERENT from neutrons because...

• One is in the nucleus, the other is in the orbitals/cloud.

• One has a charge, the other does not.

• Both are in the nucleus.

Multiple Choice

WHAT IS THE ATOMIC NUMBER OF OXYGEN?

• 16

• 8

• 15.9999

• 9

​What is an Isotope?

​Isotopes have the same number of protons (so they are the same element)

​But different numbers of Electrons

​Mass No = No of Protons + No of Neutrons

​Since Protons and Neutrons are the only subatomic particles with mass, all the mass of the atom is in the nucleus of the atom.

​Remember, Neutrons have a mass of 1 AMU

But the have no charge

Isotope Symbols

As you can see to the right there are certain ways elements and isotopes are represented as symbols. There is the element symbol (the biggest part). Then the upper number will the the mass number (number of protons + number of neutrons) and the lower number is just the atomic number (number of protons).

Multiple Choice

What makes up most of the mass of an atom?

• Electrons in the electron cloud

• only Protons have mass

• The Protons and Neutrons which are in the nucleus

• The Protons and Electrons which are in the nucleus

Multiple Choice

You find out that an atom has 5 protons, 6 neutrons, and 5 electrons. What is this atom's atomic number?

• 5

• 6

• 11

• 1

Multiple Choice

All the isotopes of a particular element will always have the same -

• Atomic number

• Mass number

• Number of neutrons

• Total number of subatomic particles

Multiple Choice

How many neutrons does the isotope of lithium - 8 have?

• 8

• 3

• 4

• 5

Ion Notation

• Same as isotope

• includes charge in upper right

• + means LESS ELECTRONS than PROTONS

• (-) means MORE ELECTRONS than PROTONS

​Let's review our electric hotel for electrons

​You are the desk clerk....

​

Check in Fluorine​

Multiple Choice

Write the shorthand electron configuration for Ca

• 1S²2S²2P⁶3S²3P⁶4S²

• [Kr]4S²

• [Ar]4S²

• [Ar)2P²

Periodic Table

By Craig LaPerriere

Multiple Choice

What is a group

• Up and down row on the table

• Up and down column on the table

• Side to side row on table

• Side to side column on the table

Multiple Choice

What is a period

• Up and down row on the table

• Up and down column on the table

• Side to side row on table

• Side to side column on the table

Multiple Choice

Which element is a Halogen?

• Argon

• Iodine

• Calcium

• Sodium

Multiple Choice

Group 18

• Alkali Metals

• Alkaline Earth Metals

• Rare Earth Metals

• Noble Gases

• Halogens

Multiple Choice

Group 1

• Alkali Metals

• Alkaline Earth Metals

• Rare Earth Metals

• Noble Gases

• Halogens

Multiple Choice

Halogens have how many valence electrons

• 1

• 2

• 7

• 8

​Valence electrons:

​The electrons in an atom’s outermost orbitals; determine the chemical properties of an element.​

-Each group of representative elements (1,2, 13-18) have an assigned amount of valence electrons.

Multiple Choice

Order the following elements in terms of increasing electronegativity

F, At, I, Cl,

• F, Cl At, I

• At, F, Cl, I

• At, I Cl, F

• F, Cl, I , At

Multiple Choice

Elements in the same family have similar _______________.

• Protons
• Physical and Chemical Properties
• Shape
• Size

Multiple Choice

Consider Fluorine's (F) location on the periodic table. Is it a metal, nonmetal, or metalloid?

• metal

• nonmetal

• metalloid

Ionic Bonding

• Occurs when a valence electron is transferred from a metal to a nonmetal

• The resulting charge difference holds them together

Naming ionic compounds is pretty simple.

• Cation + Anion = ionic compound

Metal + Nonmetal

• The metal or Cation is capitalized

• The nonmetal or Anion is not capitalized

• Change the Nonmetal ending to -ide

• Sodium chloride

Multiple Choice

Lithium Chloride

• LiCl

• Li₃Cl

• LiClO₃

• LiClO₄

Multiple Choice

 Which of the following is the correct formula for these two ions:
Al⁺³ +  S^-2

• AlS₃

• Al₂S₃

• Al₃S₂

• Al₃S

Multiple Choice

Write the formula for barium + nitrogen

• Ba₂N₃

• Ba₃N₂

• BaN

• BaN₃

Transition Metals

• Some transition metals can have more than 1 stable Cation.

• Examples

• Iron can have a 2+ or a 3+ charge

• Copper can have a 1+ or 2+ charge

Naming compounds with Transition Metals

• Use a roman numeral after the cation to show the charge of the transition metal

• Fe³⁺ is named Iron (III)

• Fe²⁺ is named Iron (II)

• Everything else stays the same

Multiple Choice

FeO

• Iron (II) Oxide

• Iron (III) Oxide

• Iron Oxide

• Iron Oxygen

Multiple Choice

Copper (II) Chloride

• CuCl₃

• CuCl₂

• Cu₂Cl

• CuClO₃

Multiple Choice

Cobalt (II) Oxide

• Co₂O

• CoO₂

• CoO

• Co₂O₂

Polyatomic Ions

• Covalently bonded compounds which have lost or gained electrons, ionizing them.

• Naming ionic compounds with polyatomic ions is easy!

• Example

• Na⁺ + SO₄ ^2- --> Na₂SO₄

• Sodium ion + Sulfate ion

• Sodium sulfate

• Mg²⁺

• SO₄^2-

• MgSO₄

• Could also be written as Mg(SO₄)

• Parenthesis are optional unless you have more than 1 SO₄^2-

• EX Pb⁴⁺ + SO₄^2- --> Pb(SO₄)₂

• Lead (IV) sulfate

Multiple Choice

Co⁺²  combines with NO₂^-  to form

• Co₂(NO₂)

• Co(NO₂)₂

• NO(Co)₂

• Co(NO)₃

Multiple Choice

Iron (II) Phosphate

• Fe₃(PO₄)₂

• FePO₄

• Fe(PO₄)₂

• Fe₃P₂

Multiple Choice

AlPO₄

• Aluminum Phosphide

• Aluminum Phosphoxide

• Aluminum Phosphorus Oxide

• Aluminum Phosphate

Match

Match the following

• negative charge

• positive charge

• atom with a charge

Anion

Cation

Ion

• Anion

• Cation

• Ion

Multiple Choice

Ionic bonds form between:

• a metal and a nonmetal

• two nonmetals

• two metals

• a metal and a noble gas

• a nonmetal and a noble gas

Naming compounds:

• ionic = name of the metal + name of the non-metal with suffix -ide

• covalent = number of atoms prefix+element name + number of atoms prefix+element with -ide root

Multiple Choice

What is the formula for diphosphorus pentoxide?

• P₂O₅

• PO₅

• P₅O₂

• P₂O₆

Multiple Choice

What is the name of N₂O₃

• Nitrogen trioxide

• Dinitrogen oxide

• Dinitrogen trioxide

• Nitrogen oxide

Multiple Select

Compounds that begin with a H are acids.

• True

• False

Multiple Choice

What is the name of HBr?

• bromic acid

• hydrobromic acid

• hydroxybromic acid

• hydroic acid

Balancing Chemical Equations

As you fill in your notes sheet, look for the BOLD RED text.

Multiple Choice

The substances that go into a reaction are called the _______.

• products

• reactants

Multiple Choice

So, the Law of Conservation of Mass would tell us that the mass of all the REACTANTS must __________ the mass of all PRODUCTS in a chemical reaction.

• equal

• be greater than

• be less than

2H₂ + O₂ ---> 2H₂O

This equation is BALANCED on both sides.

Notice that there are 4 Hydrogens and 2 Oxygens on each side.

The full-size numbers to the LEFT of the elements/compounds are called COEFFICIENTS and are the ONLY VALUES YOU CAN CHANGE.

The small numbers to the right of the elements are called SUBSCRIPTS and MUST STAY THE SAME in the equation.

Multiple Choice

What is the left part of a chemical equation called?

2H₂ + O₂ ---> 2H₂O

• Reactants

• Yields

• Products

• Chemical equation

Multiple Choice

What is the right part of a chemical equation called?

2H₂ + O₂ ---> 2H₂O

• Reactants

• Yields

• Products

• Chemical Equation

Multiple Choice

How many Oxygens are in this molecule? 
(OH)₂

• 4
• 1
• 2
• 3

Multiple Choice

What coefficients are needed to balance the equation?

___Al + ___ O₂ ---> 2Al₂O₃

• 3,2

• 3,4

• 4 , 3

• 4,2

Multiple Choice

Balance the following equation:

___ H₂+ ___ O₂→___ H₂O

• 1, 1, 3

• 2, 2, 2

• 1, 2, 1

• 2,1, 2

Multiple Choice

Pb(NO₃)₂  +  KI --> PbI₂ + KNO₃
What type of reaction is this? 

• Synthesis 
• Decomposition 
• Single Replacement
• Double Replacement 

Multiple Choice

Zn + H₂S --> ZnS + H₂

• synthesis
• combustion
• single replacement
• double replacement

Multiple Choice

CH₄ + O₂ --> CO₂ + H₂O 

• single replacement
• double replacement
• acid base
• combustion

Multiple Choice

Mg + HCl --> MgCl₂ + H₂

• combustion
• synthesis
• decomposition
• single replacement