Segment 1 Exam Review 
This review is neither a replica of the exam nor does it contain every concept in the module or what may be on the exam.  It is always best practice to review all lessons and assessments. Resubmitting is a great way to review/learn and improve your grade.   The number in parenthesis corresponds to the lesson for that question.  Please reach out to your instructor with any questions (Answer key).

The Element Song!

Be sure to go through all the module exam reviews as well!

Regular: There are 20 multiple choice questions on the exam. There are no free response/essay questions.
Honors:  There are 25 multiple choice questions on the exam. There are no free response/essay questions.
Regular:

1.	What makes something a science?  (1.01)

2.	What types of questions cannot be answered by science? (1.01) 

3.	How can we increase the scientific reliability of scientific claims? (1.01)  

4.	What are the SI units for mass, temperature, length and volume. (1.02)

5.	Which state of matter fills the entire container? (1.04)

6.	Compare and contrast physical and chemical properties.  Give a few examples of each. (1.04) 

7.	Compare a physical change with a chemical change. List a few examples of each. (1.05) 

8.	Compare a mixture and a compound. (1.06)

9.	List 4 types of equipment commonly found in the lab and identify what it measures.  What equipment do we need to determine the density of a liquid? (1.07)

10.	List the 5 statements of Dalton’s Atomic Theory. (2.01)

11.	Which scientists further evolved Bohr’s model of the atom? (2.01) Note: Be sure to be able to describe all scientists and their experiments and what they concluded.

12.	Describe the implications of Rutherford’s experiment. (2.01)

13.	Describe the implications of Thomson’s cathode ray experiment. (2.01) 

14.	Describe characteristics of metals and nonmetals. (2.02)

15.	How many orbitals are in the f sublevel? (2.03) 

16.	Draw and label an electromagnetic wave (2.04) 

17.	What do electromagnetic waves of light consist of? (2.04)

18.	If an electron increases its energy value, in J, what is the respective transition within the atom? (2.05) 

19.	What happens to the energy of electrons as we increase energy levels? (Mod 2)

20.	What is the group number of the following element: 1s2 2s2 2p6 3s2 4s2? (3.01)
a.	Group 2		c. Group 4
b.	Group 14		d. Group 18

21.	Which of the following is the correct description of an ionic bond? (3.03)
a.	Electrons are shared between atoms so that stable electron configurations are achieved
b.	An ionic bond exists between elements with large electronegativity differences
c.	An ionic bond exists between two nonmetals
d.	An ionic bond experiences very small differences in electronegativity values

22.	When one atom of lithium (Li) combines with one atom of chlorine (Cl), their bonding results in a molecule of LiCl. Which of the following describes the arrangement of valence electrons in a bond between Li and Cl? (3.03)
a.	The valence electrons spend more time around Li
b.	The valence electrons are given up by the Li and gained by the Cl
c.	The valence electrons are shared equally between Li and Cl
d.	These two atoms will not form a bond

23.	Which of the following would form an ionic bond when combined? (3.03)
a.	Hydrogen and helium
b.	Carbon and hydrogen
c.	Aluminum and oxygen
d.	Aluminum and iron

24.	Which ion would form a bond with a one-to-one ratio with a single carbonate polyatomic ion? (3.03)
a.	Na+			c. Li+
b.	Mg+2			d. P+3

25.	What is the formula of a compound formed between magnesium and oxygen? (3.03)
a.	MgO			c. Mg2O2
b.	MgO2			d. OMg

26.	Which of the following is not a correct formula unit? (3.03)
a.	AlP			c.  NaF
b.	CaS2			d.  HF

27.	The Lewis Dot Structure of a molecule is written below.  Which of the following is correct? (3.04)

a.	The sulfur atom has two non-bonded pairs and one bonded pair of electrons.
b.	The electronegativity difference between hydrogen and sulfur is greater than 1.7.
c.	The octet of electrons on the sulfur atom remains incomplete in the molecule.
d.	The sulfur atom has two lone pairs of electrons and two single bonds.

28.	Describe the electrons around each oxygen in the following molecule (3.04): 

a.	Each oxygen atom has 6 electrons around it
b.	Each oxygen atom has 2 bonded pairs of electrons and 2 non-bonded pairs of electrons
c.	Neither oxygen atom follows the octet rule
d.	Each oxygen atom has 2 non-bonded pairs of electrons and 1 shared pair of electrons

29.	A molecule has two bonded atoms around the central atom. The central atom has one lone pair. What is the geometry of the molecule? (3.05)
a.	Bent			c. Trigonal planar
b.	Tetrahedral		d. Linear

30.	Which of the following is NOT true about hydrogen bonding? (3.06)
a.	It is an intermolecular force
b.	It exists between any element and hydrogen.
c.	It is the strongest of all the intermolecular forces.
d.	Water experiences hydrogen bonding.

31.	Electrostatic attraction of permanent dipoles in polar molecules is a definition of which type of intermolecular force? (3.06)
a.	London Dispersion	c.  Dipole-Dipole
b.	Ion-Dipole		d.  Hydrogen Bonding

32.	How many oxygen atoms should appear on the right side of the following equation? (4.01)			Al(NO3)3 + 3NaOH  →
a.	Three			c. Six
b.	Nine			d. Twelve

33.	Two reactions occur as follows:
Reaction A:  Element + oxygen gas forms one compound
Reaction B: Ionic compound + ionic compound forms two compounds

Which of the following is true? (4.02-4.04)

a.	A is a synthesis reaction and B is a single replacement
b.	A could be classified as a redox reaction, but not B
c.	Neither reaction is a combustion reaction
d.	A is a single replacement reaction and B could be a synthesis

34.	Which of the following reactions could be classified as three different types? (4.02 - 4.04)
a.	2Fe + 3CuSO4 → Fe2(SO4)3 + 3Cu
b.	2Mg + O2  →2 MgO
c.	FeS + 2HCl → H2S + FeCl2
d.	2NaN3 → 2Na + 3N2
35.	Which of the following can be true for a redox reaction? (4.04) Note: Be sure you can explain the characteristics of all seven types of reactions in lessons 4.02 - 4.04 as well as their reactants, products and be able to give an example.
a.	Oxygen is always a reactant
b.	One product is always formed
c.	The oxidation state of one reactant changes
d.	At least one atom gains electrons and one atom loses electrons

36.	What is the best description of a nuclear reaction? (4.05)
a.	The atoms change who they are bonded to.
b.	The number of protons changes in an element thus changing its identity
c.	Atoms change the number of electrons or their oxidation number
d.	They produce less energy than chemical reactions.

Honors Extension: 

37.	(1.03H) List and describe two pseudosciences.

38.	(1.03H) What is true for a hypothesis, but not a scientific theory?

39.	(2.06H) Which of the following is incorrect in describing effective nuclear charge? 
a.	It is affected by the number of shielding electrons
b.	It generally increases across a period
c.	It is the number of core electrons minus the number of valence electrons
d.	It remains relatively constant down a group

40.	(3.07H) A carbon atom is able to form four single covalent bonds because it: 
a.	Has four electrons and four protons.
b.	Has four valence electrons in its outermost energy level.
c.	Forms a polyatomic ion with a -4 charge.
d.	Forms a more stable isotope when it gains four more electrons. 

41.	(3.07H) The organic compounds that are structural elements in the cell walls of plants and bacteria are known as: Note: Be familiar with all the functional groups.
a.	Carbohydrates		c. Polymers.
b.	Hydrocarbons		d.  Alcohols

42.	(3.07H)  The table shows the properties of some organic compounds.

Compound A	Compound B	
Usually has an aldehyde or a ketone and a hydroxyl group	Has a carbon atom is double-bonded to a nitrogen atom	

Which statement best identifies compounds A and B?

a.	Compound A is a ketone and Compound B is a polymer
b.	Compound A is a carbonyl group and Compound B is an amine
c.	Compound A is an alcohol  and Compound B is a carbonyl group
d.	None of the above

43.	(4.06H) Which of the following governs nuclear decay?  (Be sure to study pg 2 of the lesson)
a.	Strong nuclear			c.  Weak nuclear
b.	London Dispersion		d.  Gravity

44.	(4.06H) Which of the following fundamental forces acts only between charged particles? 
a.	Weak nuclear			c.  Gravity
b.	Electromagnetism		d.  Hydrogen bonding

45.	(4.06H) What happens to the amount of carbon-14 after an organism dies?
a.	It increases				c. It decreases
b.	It doesn’t effect the C12/C14 ratio	d. It is unknown.