Final exam Review part 1

Something that you have learned by seeing or watching something and thinking about it.
A. Theory
B. Law
C. Observation
D. Expiriment

​Example question

o   Know definitions of hypothesis, observation, theory and law 

o    Differentiate observations from theories from laws:

• A Law is an observable relationship between 2 values. 

• A Theory is an explanation to explain why the relationship exists.

• A Hypothesis is an explanation that is not yet supported by a lot of evidence.

 

​Chapter 1

Chapter 1-6 The Student should be ablt to:

Something that you have learned by seeing or watching something and thinking about it.
A. Theory
B. Law
C. Observation
D. Expiriment

​Example question

o   Know definitions of hypothesis, observation, theory and law 

o    Differentiate observations from theories from laws:

• A Law is an observable relationship between 2 values. 

• A Theory is an explanation to explain why the relationship exists.

• A Hypothesis is an explanation that is not yet supported by a lot of evidence.

 

​Chapter 1

Chapter 1-4 The Student should be ablt to:

Chapter 2

• Write a number in scientific notation.

• Use the density formula to solve for density, mass, or volume

• Use conversion factors to change from one unit to another (dimensional analysis)

• Convert a measurement from one metric unit to another

• Slove multifunction problems and answer using the correct number of significant figures

Multiple Choice

A mechanical pencil has the density of 3.000 g/cm³.  The volume of the pencil is 15.8 cubic centimeters.  What is the mass of the pencil?

• 47.4 g
• 50 g
• 0.190  g
• 5.27 g

Multiple Choice

Write 3.2 x 10³ in standard form.

• 3.200
• 3200
• 32000
• .0032

Multiple Choice

Write 9,450,000 in scientific notation.

• 9.45 x 10⁴
• 9.45 x 10⁵
• 9.45 x 10⁶
• .945 x 10⁷

Math Response

How many micrometers in .03891 centimeters?

Type answer here

Correct Answer: 389.1

Deg^°

Rad

Sig figs when adding/subtracting

When adding or subtracting, round your answer to the same place as the number with the LEAST amount of DECIMALS.

​45.879 + 32.1 = 77.979

​45.879 + 32.1 = 77.979​ ------> 78.0

​5.41 + 65.456 = 70.866

​​5.41 + 65.456 = 70.866 -------> 70.87

​Sig figs when multiplying/dividing

When multiplying or dividing, round your answer to the same place as the number with the LEAST amount of SIGNIFICANT FIGURES.

​47.06 x 1.0004 = 47.078824

​​47.06 x 1.0004 = 47.08

​98.04​ = 32.68

3​

​​98.04​ = 30

3​

Math Response

Solve the following equation as written using the correct number of sig figs

(876.90+98.1)/56.998

Type answer here

Correct Answer: 17.11

Deg^°

Rad

Multiple Choice

How many significant figures?

7945

• 1

• 2

• 3

• 4

Multiple Choice

How many significant figures does the following number have: 0.002040?

• 6

• 4

• 3

• 2

Chapter 3

• Differentiate chemical and physical properties of matter (chemical change: one or more substances making or breaking bonds and forming a new substance)

• Classify matter as a pure substance or a mixture.

• Differentiate homogeneous mixtures and heterogeneous mixtures 

• Use specific heat to calculate heat loss or gain, temperature change, or mass of a sample

Multiple Choice

Ability to rust is this type of property:

• Physical property
• Chemical property

Multiple Choice

Boiling Point: Chemical or Physical Property

• Chemical Property
• Physical Property

Multiple Choice

Melting Point: Chemical or Physical Property

• Chemical Property
• Physical Property

Multiple Choice

Reacts with Acid: Chemical or Physical Property

• Chemical Property
• Physical Property

Multiple Choice

Type of mixture that has the SAME COMPOSITION in every part.

• Homogenous

• Heterogeneous

Multiple Choice

Type of mixture that DOESN'T HAVE the same composition in every part.

• Homogeneous

• Heterogeneous

Multiple Choice

The specific heat of aluminum is 0.903 J/g°C.  How much heat(Q) is released when a 10.0 g piece of aluminum foil is taken out of the oven and cools from 100.0° to 50.0°?

• 452 J

• 4.51 J

• 903 J

• 50 J

Chapter 4

• Given the atomic number and mass number of an atom, state the number of protons, neutrons, and electrons

• Give the number of protons, electrons, and neutrons in the isotopes of an element

• Know charge of ions that Group 1, 2, 14, 15, 16, 17, (18) elements are capable of making

• Describe the electrical charge and location in an atom of a proton, a neutron, and an electron

Multiple Choice

Group 17 (7A) always has ions with a charge of 

• +1
• +2
• -1
• -2

Multiple Choice

How many electrons does a Na⁺¹ ion have?

• 12

• 11

• 10

• 9

Multiple Choice

Which of the following elements is an alkali metal?

• calcium

• magnesium

• mercury

• sodium

Multiple Choice

Which group is very stable due to the fact that they have a full outermost energy level?

• alkali metals

• halogens

• alkaline-earth metals

• noble gases

Multiple Choice

Who created the plum pudding model of the atom?

• Rutherford and the plums were protons

• Rutherford and the plums were electrons

• Thomson and the plums were protons

• Thomson and the plums were electrons

Multiple Choice

Rutherford realized that the atomic nucleus was positively charged because

• it attracted alpha particles.

• it deflected alpha particles.

• it had no effect on alpha particles.

• it produced alpha particles.

Multiple Choice

Based on Rutherford's model of the atom, electrons in the atom are located

• inside of the nucleus of the atom

• outside and around the nucleus of the atom

• outside and inside of the nucleus of the atom

Multiple Choice

Added energy levels to the atom model

• Antione Lavoisier

• Niels Bohr

• JJ Thomson

• James Chadwick

Chapter 5

• Use chemical formulas to classify compounds and molecules as ionic or covalent

• Write the names and formulas of compounds

• Use charge to establish the ratio of elements in an ionic compound

• Use the name of a covalent compound to establish the ratio of elements.

Multiple Choice

Ionic compounds generally form when ____________ and ________________ react with each other.

• nonmetals and nonmetals
• metals and metals
• metals and nonmetals
• polyatomic elements & nonmetals

Multiple Choice

How many total electrons are in an oxide ion (O^2-)?

• 10
• 8
• 6
• 0

Multiple Choice

Which of the following is the correct name for the chemical formula Li₂S?

• Lithium sulfate
• lithium sulfide
• lithium sulfite
• lithium hyposulfite

Multiple Choice

copper(II) chloride

• CuCl₂
• CuCl
• Cu₂Cl
• Cu₂Cl₂

Multiple Choice

What is the formula for calcium phosphide?

• CaP
• Ca₂P₃
• Ca₃P₂
• Ca₂P

Multiple Choice

Carbon dioxide

• C₂O₂
• C₂0
• CO
• CO₂

Multiple Choice

Phosphorous trichloride

• PCl₃
  
• P₃Cl
• P₃Cl₃
• PCL

Multiple Choice

P₂O₅

• Phosphorus Oxide
• Pentaphosphorus Dioxide
• Diphosphorus pentoxide

• Phosphoric Oxygen

Multiple Choice

CO

• Carbon Oxide
• Carbon Oxygen
• Dicarbon dioxide
• Carbon Monoxide

Multiple Choice

What is the name of Ca(NO₃)₂

• calcium dinitrite

• calcium II nitrate
• calcium nitrate
• carbon nitrate

Multiple Choice

An ionic compound made of copper (Cu²⁺) and oxygen would be named

• copper oxygen.
• copper oxide.
• dicopper oxide.
• copper(II) oxide.

Multiple Choice

Fe⁺³ combines with S^-2 to form 

• Fe⁺⁴(S)⁼³
• Fe²S⁴
• Fe₂S₃
• Fe³S²

Multiple Choice

copper(II) chloride

• CuCl₂
• CuCl
• Cu₂Cl
• Cu₂Cl₂

Chapter 6

• Define: mole, Avogadro’s number, molar mass, mole ratio, percent composition, empirical formula, molecular formula

• Use Avogadro’s number to convert between particles (atoms, molecules, or formula units) and moles (A mole is a set of 6.022*10²³ items (Avogadro’s number) that is handy to use in chemistry because a mole of particles has the same mass in grams as one particle has in amu’s.)

• Given the chemical formula of a substance, calculate its molar mass in grams per mole (g/mol)

• Use molar mass to convert between mass and moles for an element and for a compound

• Use a mole ratio to convert between moles of a compound and moles of an element within the compound (1 mol CH₄ = 4 mol H)

• Perform multi-step conversions

Multiple Choice

How many moles are in 8.30 X 10²³ molecules of H₂O?

• 1.38 X 10²³ moles H₂O

• 1.38 moles H₂O

• 2 moles H₂O

• 1 mole H₂O

Multiple Choice

How many molecules are there in 31.8 moles of water?

• 5.28 x 10^-23 molecules

• 1.91 x 10²⁵ molecules

• 5.28x 10^-25 molecules

• 1.91 x 10²³ molecules

Multiple Choice

How many grams are in 10 mol of fluorine?

• 19 grams

• 190 grams

• 90 grams

• 9 grams

Multiple Choice

What are the units for molar mass?

• squirrels

• amu

• grams/mole

• liters

Multiple Choice

What is the percent composition of Carbon in C₂H₄?

• 86%

• 50%

• 33%

• 43%

Multiple Choice

What is the empirical formula for the following:

32.40% sodium, 22.5% sulfur; 45.1 % oxygen, 37.75% water?

• Na₂SO₄H₆O₃

• Na₂SO₄ * 2H₂O

• Na₂SO₄ * 3H₂O

• Na₂SO₄ * (H₂O)

Multiple Choice

What is the molecular formula if the empirical formula is CH₂O and the molecular molar mass is 180.18?

• CH₂O
• C₂H₄O₂
• C₄H₈O₄
• C₆H₁₂O₆

Multiple Choice

How many moles are in 16.9g of water?

• 16.9 mol H₂O

• 305. mol H₂O

• .938 mol H₂O

• 1.06 mol H₂O

Multiple Choice

Find the number of moles in 25.0 grams of HF?

• .760 mol HF

• 25 mol HF

• 1.25 mol HF

• 80 mol HF