Chemistry Mr. Kalkman Name:
Midterm Review Stations Date:
Atomic Structure
Directions: Oxygen has 3 naturally occurring Isotopes. O-16 has a relative abundance of 99.74%, O-17 has a naturally abundance of 0.037% and O-18 has a natural abundance of 0.205%. Using the following diagram, create an atomic model for the least common isotope of oxygen. Use circles to represent the subatomic particles, and use the circles at the top to make a key. Include the proper number of each type of subatomic particle.
On the back, calculate the average atomic mass of oxygen.
Blue Green Red
Chemistry Mr. Kalkman Name:
Midterm Review Stations Date:
Chemistry Math
- How many Significant Figures do each of the following numbers have?
- 0.502
- 29030
- 5.68900
- 0.00001234
- Convert the following numbers into scientific notation.
- 0.000002305
- 60200000
- 10932098235
- 0.00000000012
- Perform the following operations and record your answer the proper number of Sig Figs.
- 5.60 + 2.789
- 9.122 – 0.5020
- 3.75 x 0.46
- 10.23 / 3.2
- What is the % composition of Oxygen in the following compounds?
- MgO
- Na2O
- H2O
- CO2
- Convert the following units.
- 50mL à ? L
- 1009768 mg à ? kg
- 0.78 km à ? cm
- 2.32 kJ à ? J
Chemistry Mr. Kalkman Name:
Midterm Review Stations Date:
Thermodynamics
Directions: On the following graph, draw in an appropriate scale for the y axis and label the scale on the x axis. Include the Melting and Boiling Points. Label the location for any phases included in the graph as well as the name of any phase changes. For the follow up questions, use the back if you need more space.
A beaker containing 100g of ice is heated at a constant rate for 5 minutes until it begins to melt. After 2 minutes, the ice is now water and is heated until it begins to boil 6 minutes later. After 10 minutes of boiling, no water remains in the beaker.
1. How much heat is absorbed by the water during the first three minutes it is only a liquid.
2. How much heat is absorbed by the water during the 2 minutes it is melting?
Chemistry Mr. Kalkman Name:
Midterm Review Stations Date:
Famous Experiments
Ernest Rutherfordpublishes his atomic theory describing the atom as having a central positive nucleus surrounded by negative orbiting electrons. This model suggested that most of the mass of the atom was contained in the small nucleus, and that the rest of the atom was mostly empty space. Rutherford came to this conclusion following the results of his famous gold foil experiment. This experiment involved the firing of radioactive particles through minutely thin metal foils (notably gold) and detecting them using screens coated with zinc sulfide. Rutherford found that although the vast majority of particles passed straight through the foil approximately 1 in 8000 were deflected leading him to his theory that most of the atom was made up of empty space.
J.J. Thomson’s experiments suggested not only that cathode rays (electrons) were over 1000 times lighter than the hydrogen atom, but also that their mass was the same whatever type of atom they came from. He concluded that the rays were composed of very light, negatively charged particles which were a universal building block of atoms. He called the particles "corpuscles", but later scientists preferred the nameelectronwhich had been suggested byGeorge Johnstone Stoneyin 1894, prior to Thomson's actual discovery. In April 1897 Thomson had only early indications that the cathode rays could be deflected electrically. A month after Thomson's announcement of the corpuscle he found that he could deflect the rays reliably by electric fields if he evacuated the discharge tubes to very low pressures.
Questions on Back à
1. What were the conclusions of the Gold Foil Experiment?
2. What were the conclusions of the Cathode Ray Experiment?
3. Describe what the first picture is showing.
4. Describe what the second picture is showing.
5. Describe what the third picture is showing.
Chemistry Mr. Kalkman Name:
Midterm Review Stations Date:
Periodic Table
1 An element that has a low first ionization energy and good conductivity of heat and electricity is classified as a
(1) metal (3) nonmetal
(2) metalloid (4) noble gas
2 The chemical properties of calcium are most similar to the chemical properties of
(1) Ar (3) Mg
(2) K (4) Sc
3 Which element is a liquid at STP?
(1) argon (3) chlorine
(2) bromine (4) sulfur
4 Which statement describes a chemical property of aluminum?
(1) Aluminum is malleable.
(2) Aluminum reacts with sulfuric acid.
(3) Aluminum conducts an electric current.
(4) Aluminum has a density of 2.698 g/cm3 at STP.
5 As atomic number increases within Group 15 on the Periodic Table, atomic radius
(1) decreases, only
(2) increases, only
(3) decreases, then increases
(4) increases, then decreases
6 A sample of an element is malleable and can conduct electricity. This element could be
(1) H (3) S
(2) He (4) Sn
7 Which general trend is demonstrated by the Group 17 elements as they are considered in order from top to bottom on the Periodic Table?
(1) a decrease in atomic radius
(2) a decrease in electronegativity
(3) an increase in first ionization energy
(4) an increase in nonmetallic behavior
8 Which element is a liquid at 758 K and standard pressure?
(1) gold (3) platinum
(2) silver (4) thallium
9 An element that is malleable and a good conductor of heat and electricity could have an atomic number of
(1) 16 (3) 29
(2) 18 (4) 35
10 An atom of an element has a total of 12 electrons. An ion of the same element has a total of 10 electrons. Which statement describes the charge and radius of the ion?
(1) The ion is positively charged and its radius is smaller than the radius of the atom.
(2) The ion is positively charged and its radius is larger than the radius of the atom.
(3) The ion is negatively charged and its radius is smaller than the radius of the atom.
(4) The ion is negatively charged and its radius is larger than the radius of the atom.
11 Which electron configuration represents an atom in an excited state?
(1) 2–7 (3) 2–8–1
(2) 2–6–2 (4) 2–8–8–2
12 At standard pressure, which element has a freezing point below standard temperature?
(1) In (3) Hf
(2) Ir (4) Hg
13 On the modern Periodic Table, the elements are arranged in order of increasing
(1) atomic mass (3) mass number
(2) atomic number (4) oxidation number
14 An atom of an element forms a 2+ ion. In which group on the Periodic Table could this element be located?
(1) 1 (3) 13
(2) 2 (4) 17
15 Which Group 14 element is a metalloid?
(1) tin (3) lead
(2) silicon (4) carbon
Chemistry Mr. Kalkman Name:
Midterm Review Stations Date:
Matter
1 Which substance can be broken down by chemical means?
(1) magnesium (3) manganese
(2) mercury (4) methanol
2 Which statement describes oxygen gas, O2(g), and ozone gas, O3(g)?
(1) They have different molecular structures, only.
(2) They have different properties, only.
(3) They have different molecular structures and different properties.
(4) They have the same molecular structure and the same properties.
3 Which statement describes a chemical property of bromine?
(1) Bromine is soluble in water.
(2) Bromine has a reddish-brown color.
(3) Bromine combines with aluminum to produce AlBr3.
(4) Bromine changes from a liquid to a gas at 332 K and 1 atm.
4 Which type of matter is composed of two or more elements that are chemically combined in a fixed proportion?
(1) solution (3) homogeneous mixture
(2) compound (4) heterogeneous mixture
5 Matter is classified as a
(1) substance, only
(2) substance or as a mixture of substances
(3) homogenous mixture, only
(4) homogenous mixture or as a heterogeneous mixture
6 Which substance can not be decomposed by a chemical change?
(1) ammonia (3) copper
(2) propanol (4) water
7 A beaker contains both alcohol and water. These liquids can be separated by distillation because the liquids have different
(1) boiling points (3) densities
(2) particle sizes (4) solubilities
8 An unknown substance has a mass of 10.65 g and a volume of 3.45mL. What is its Density? Will this substance float in water?
9 If a sample of Iron has a mass of 36.7 g, what is its volume?
10 If a sample of Copper has a volume of 98.5mL, what is its mass?