Semester Review

Rules

• Whiteboard must have team # on top and questions must be numbered and written legibly

• Each person on the team must write in a different color marker, team members can NEVER switch markers

• YOU MAY NOT ANSWER SOMEONE ELSES QUESTION OR CORRECT SOMEONE ELSES QUESTION – this will disqualify your entire team

• After Ms. Hubbell says- COMMUNICATE!, THEN you may help each other on a question

• At the end – 1st place receives 5 pts extra credit, 2nd place receives 2.5 pts extra credit, 3rd place receives 1 pt extra credit

States of matter

• Which of the above represents..1. An element in the liquid state?2. A mixture of elements and compounds?3. A mixture of elements?4. An element in the solid state?

Physical/Chemical change

1. What is the difference between a physical and chemical change?

• Are the following physical or chemical changes?2. Burning of paper

3. Melting of ice cube

4. Sand turning into glass when being struck by lightning

Conservation of Matter

1. What does the conservation of matter state?

2. Given the following equation, how many grams of Chlorine gas are used in the reaction if 29 g of Na react with Cl2 to form 35 g of NaCl?

– 2Na + Cl2 2NaCl

3. Which two subatomic particles have mass?

4. Which two subatomic particles have a charge?

The Atom

1. In 16O, what does the number 16 stand for? What does the number 8 stand for?

2. Has how many protons does 16O have?

3. How many neutrons does 16O have?

4. How many electrons does 16O have?

C146

8

8

8

8

The Atom

1. How is an ion different from an atom?2. When metals form a charge, they

__________ electrons. When nonmetals form a charge, they ___________ electrons.

3. How many electrons does an N-3 ion have?

4. How many electrons does a Na+1 ion have?

Mass Number/Avg. Atomic mass

1. What is the mass number of hydrogen-1?

2. What is the average atomic mass of hydrogen?

3 & 4. Calculate the average atomic mass for the element zyrton with two isotopes: one with a mass of 154 amu and an abundance of 10.05% and the other with a mass of 155 amu and a mass of 89.95%.

Scientists

1. List one of Dalton’s 4 postulates.

2. List a second postulate of Dalton (different than the first).

3. List a third postulate of Dalton.

4. List a fourth postulate of Dalton.

Scientists

1. What did Thompson’s model look like?

2. What did Rutherford’s gold foil experiment prove?

3. How did Bohr come up with his planetary structure?

4. What is our most current model of the atom?

Electron Configuration

1. What is the electron configuration for Copper?

2. What does the numbers 1,2,2,3… stand for in the above answer?

3. What do the letters s,p,d,f stand for

4. What do the superscripts stand for?

Periodic table

1. The rows across the periodic table are ________ and the columns up and down are called _________.

2. Describe where to find the metals. Give 2 properties of metals.

3. Describe where to find the nonmetals. Give 2 properties of nonmetals.

4. Describe where to find the semimetals. Give 2 properties of semimetals.

Periodic Table

1. In what group are the alkali metals?

2. In what group are the halogens?

3. In what group are the noble gases?

4. What “block” contains the transition metals? What “block” contains the inner transition metals?

Periodic trends1. Atomic radius ___________ as you move

across a period and _________ as you go down a group.

2. Ionization energy ___________ as you move across a period and _________ as you go down a group.

3. Electronegativity ___________ as you move across a period and _________ as you go down a group.

4. What element has the highest Electronegativity?

Nuclear Decay

1. The force that holds the nucleus together is called the _________________.

2. What are the three types of nuclear decay?

3. Question: Balance the following reaction

88Ra 2He + ?

4. What is the most dangerous type of radiation?

226 4

226 4

Valence Electrons/ Charges

1. How many valence electrons does sodium have?

2. How many valence electrons does silicon have?

3. What kind of charge would fluorine have if it formed an ion?

4. What kind of charge would magnesium have if it formed an ion?

Ionic/Molecular compounds

1. A molecular compound is made up of a ___________ combined with a _________.

2. An ionic compound is made up of a _________ combined with a ___________.

3. Give an example of two elements that could combine to form an ionic compound.

4. Give an example of two elements that could combine to form a molecular compound.

Molecular/Ionic Compounds

1 & 2: What are 2 properties of molecular compounds?

3 & 4: What are two properties of ionic compounds?

Molecules & Polarity

1. What shape is NCl3 shown below?

2. What is the molecule polarity of NCl3?

3. What shape is CCl4 shown below?

4. What is the molecule polarity of CCl4?

Naming Compounds

Give names for the following formulas:1. NaBr

2. FeSO4

3. SiO2

4. TiCl3

Naming Compounds

• Give formulas for the following compounds:1. Dinitrogen tetraoxide

2. Lead (II) oxide

3. Manganese (IV) nitrate

4. Carbon monoxide

Chemical Equations

• Classify AND balance the following chemical equations:1. K2SO4 + BaCl2 KCl + BaSO4

2. Fe + SnCl2 Sn + FeCl23. N2 + O2 N2O3

4. CH4 + O2 H2O + CO2

Chemical equations

1. What are the seven diatomic elements?

2. What are the products of the typical combustion reaction?

3. Will the following reaction occur?– Zn (s) + Fe(NO3)2 (aq)

4. What will be the precipitate of the following reaction?– Mg(NO3)2 + KOH