|
Dalton’s Atomic Theory states |
that matter is composed of small indestructible particles |
|
The statement, "In a chemical reaction, matter is neither created nor destroyed." is called |
The Law of Conservation of Mass |
|
Which of the following represents a hypothesis? |
When a substance combusts, it combines with air. |
|
Which of the following represent a valid hypothesis? |
Metals tend to lose electrons. |
|
Choose the pure substance from the list below |
sugar |
|
Choose the pure substance from the list below. |
carbon monoxide |
|
Choose the heterogeneous mixture from the list below |
chicken noodle soup |
|
Choose the homogeneous mixture from the list below. |
kool-aid |
|
Choose the homogeneous mixture from the list below |
air |
|
Molecules can be described as |
two or more atoms joined together in a specific geometric arrangement |
|
The Scientific Method |
is based on continued observation and experiment |
|
Which of the following statements is TRUE |
A scientific law summarizes a series of related observations |
|
Which of the following statements about crystalline and amorphous solids is TRUE? |
A crystalline solid is composed of atoms or molecules arranged with long-range repeating order. |
|
Which of the following statements about the phases of matter is TRUE? |
In both solids and liquids, the atoms or molecules pack closely to one another. |
|
A substance that can’t be chemically broken down into simpler substances is considered |
an element. |
|
A substance composed of 2 or more elements in a fixed, definite proportion is considered |
a compound. |
|
Two or more substances in variable proportions, where the composition is constant throughout are considered |
a homogeneous mixture. |
|
Two or more substances in variable proportions, where the composition is variable throughout are considered |
a heterogeneous mixture. |
|
Which of the following are examples of physical change? |
All of these are examples of physical change. |
|
Which of the following are examples of physical change? |
dew forms on a blade of grass |
|
Which of the following are examples of a chemical change? |
Both a and b are examples of chemical change. |
|
Which of the following are examples of a chemical change |
leaves turning color in the fall |
|
A physical change |
occurs when sand is filtered from salt water. |
|
A chemical change |
occurs when methane gas is burned. |
|
Which of the following represents a physical property? |
Mercury is a silver liquid at room temperature. |
|
Which of the following represents a chemical property of hydrogen gas? |
It reacts explosively with oxygen. |
|
Read the water level with the correct number of significant figures. |
5.4 mL |
|
Read the temperature with the correct number of significant figures. |
87.24°C |
|
Read the length of the metal bar with the correct number of significant figures |
15.1 cm |
|
Read the length of the metal bar with the correct number of significant figures. |
15.10 cm |
|
How many significant figures are in 1009.630 mL |
7 |
|
How many significant figures are in 3.408 x 104 m? |
4 |
|
How many significant figures are in the measurement, 463.090 m? |
6 |
|
How many significant figures are in the measurement, 0.0005890 g? |
4 |
|
What answer should be reported, with the correct number of significant figures, for the following calculation? (433.621 – 333.9) × 11.900 |
1.19 × 103 |
|
What answer should be reported, with the correct number of significant figures, for the following calculation? (249.362 + 41) / 63.498 |
4.57 |
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What answer should be reported, with the correct number of significant figures, for the following calculation? (965.43 × 3.911) + 9413.4136 |
13189 |
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A student performs an experiment to determine the density of a sugar solution. She obtains the following results: 4.11 g/mL, 4.81 g/mL, 4.95 g/mL, 3.75 g/mL. If the actual value for the density of the sugar solution is 4.75 g/mL, which statement below best describes her results? |
Her results are neither precise nor accurate. |
|
A student performs an experiment to determine the density of a sugar solution. She obtains the following results: 4.71 g/mL, 4.73 g/mL, 4.67 g/mL, 4.69 g/mL. If the actual value for the density of the sugar solution is 4.40 g/mL, which statement below best describes her results? |
Her results are precise, but not accurate. |
|
If an object has a density of 8.65 g/cm3, what is its density in units of kg/m3? |
8.65 × 103 kg/m3 |
|
Determine the density of an object that has a mass of 149.8 g and displaces 12.1 mL of water when placed in a graduated cylinder. |
12.4 g/mL |
|
Determine the volume of an object that has a mass of 455.6 g and a density of 19.3 g/cm3. |
23.6 mL |
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Determine the mass of an object that has a volume of 88.6 mL and a density of 9.77 g/mL. |
866 g |
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Which of the following are examples of intensive properties? |
density |
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Which of the following are examples of extensive properties? |
mass |
|
Which of the following statements about energy is FALSE? |
Potential energy is associated with the motion of particles |
|
If the temperature is 178°F, what is the temperature in degrees celsius? |
81.1°C |
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If a solution has a temperature of 355 K, what is its temperature in degrees celsius? |
82°C |
|
All of the following are SI base units of measurement, EXCEPT |
gram |
|
What wavelength of light would you report in units of nm, if the light had a wavelength of 7.60 x 10-10 m? |
0.760 nm |
|
How many mg does a 433 kg sample contain? |
4.33 × 108 mg |
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How many kL does a 1.25 × 108 cL sample contain? |
1.25 × 103 kL |
|
How many cm3 are contained in 3.77 × 104 mm3? |
3.77 × 102 cm3 |
|
If the walls in a room are 955 square feet in area, and a gallon of paint covers 15 square yards, how many gallons of paint are needed for the room? (3 ft = 1 yd) |
7.0 gallons |
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If a room requires 25.4 square yards of carpeting, what is the area of the floor in units of ft2? (3 ft = 1 yd) |
229 ft2 |
|
kilo |
10^3 |
|
centi |
10^-2 |
|
milli |
10^-3 |
|
nano |
10^-9 |
|
micro |
10^-6 |
|
A sample of liquid isopropanol is placed in a sealed container. Some of the volatile isopropanol vaporizes. Does the mass of the sealed container and its contents change during the vaporization? Explain. |
No. The vaporized isopropanol is just in a different physical state. It still has mass and therefore the gas plus the remaining liquid and container have the same total mass after the vaporization of some of the isopropanol. |
|
What is the difference between a physical property and a chemical property? Give an example of each. |
A physical property is something that can be observed without changing the chemical identity of the substance, such as color or scent. A chemical property can only be observed while the chemical identity of a substance is changing, such as sodium metals tendency to react with water to form hydrogen gas and sodium hydroxide. |
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What does it mean to be an exact number? Give an example of an exact number. |
An exact number has an infinite number of significant figures even though we typically don’t write many of them out. If there are 26 people in a classroom, there are exactly 26.00000…. people in that room. There is no possibility of a half person, so this is an exact whole number with no ambiguity. |
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What happens to the density of a sample of iron metal as it is heated from room temperature to 100°C? (This is below the melting point of iron) |
Since the mass of the iron stays constant, but the volume increases as the temperature is raised, the density of the iron decreases upon heating. |
|
Describe the difference between an intensive and extensive property using examples. |
An intensive property doesn’t depend on the amount of the substance present, such as color or density. An extensive property is one that does depend on the amount of the substance, such as mass or volume. |
|
chapter 2 |
…NOTES |
|
What element is defined by the following information? p+ = 11 n° = 12 e- = 11 |
sodium |
|
What element is defined by the following information? p+ = 20 n° = 20 e- = 20 |
calcium |
|
What element is defined by the following information? |
chlorine |
|
What does "X" represent in the following symbol? |
bromine |
|
What does "X" represent in the following symbol? |
uranium |
|
What does "X" represent in the following symbol? |
silicon |
|
Determine the number of protons, neutrons and electrons in the following: |
p+ = 18 n° = 22 e- = 18 |
|
Determine the number of protons, neutrons and electrons in the following: |
p+ = 12 n° = 13 e- = 12 |
|
Determine the number of protons, neutrons and electrons in the following: |
p+ = 29 n° = 36 e- = 29 |
|
What species is represented by the following information? p+ = 12 n° = 14 e- = 10 |
Mg2+ |
|
What species is represented by the following information? p+ = 47 n° = 60 e- = 46 |
Ag+ |
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What species is represented by the following information? p+ = 17 n° = 18 e- = 18 |
Cl- |
|
Which of the following elements is NOT a metal? |
Xe |
|
Which of the following elements is a metal? |
Sn |
|
Which of the following elements is a nonmetal? |
P |
|
Which of the following elements is a noble gas? |
Ar |
|
Which of the following elements is a halogen? |
I |
|
Which of the following elements is an alkaline earth metal? |
Mg |
|
Which of the following elements is an alkali metal? |
Li |
|
Predict the charge that an aluminum ion would have. |
3+ |
|
Predict the charge that a calcium ion would have. |
2+ |
|
Predict the charge that an ion formed from sulfur would have. |
2- |
|
Predict the charge that the ion formed from bromine would have |
1- |
|
A 14.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3). If ammonia is the only product, what mass of ammonia is formed? |
17.03 g |
|
A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl3). If it is the only product, what mass of PCl3 is formed? |
54.93 g |
|
Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kg of iodine were produced? |
79.4 kg |
|
Two samples of calcium fluoride are decomposed into their constituent elements. The first sample produced g of calcium and g of fluorine. If the second sample produced 294 mg of fluorine, how many g of calcium were formed? |
0.309 g |
|
Calculate the atomic mass of silver if silver has 2 naturally occurring isotopes with the following masses and natural abundances: Ag-107 106.90509 amu 51.84% |
108.19 amu |
|
Calculate the atomic mass of gallium if gallium has 2 naturally occurring isotopes with the following masses and natural abundances: Ga-69 68.9256 amu 60.11% |
69.72 amu |
|
Calculate the atomic mass of element "X", if it has 2 naturally occurring isotopes with the following masses and natural abundances: X-45 44.8776 amu 32.88% |
46.27 amu |
|
How many silver atoms are contained in 3.75 moles of silver? |
2.26 × 10^24 silver atoms |
|
How many xenon atoms are contained in 2.36 moles of xenon? |
1.42 × 10^24 xenon atoms |
|
How many argon atoms are contained in 7.66 x 105 mmol of argon? |
4.61 × 10^26 Ar atoms |
|
What mass (in kg) does 5.84 moles of titanium (Ti) have? |
0.280 kg |
|
What mass (in mg) does 2.63 moles of nickel have? |
1.54 x 105 mg |
|
What mass (in g) does 3.99 moles of Kr have? |
334 g |
|
How many moles of Kr are contained in 398 mg of Kr? |
4.75 × 10^-3 moles Kr |
|
How many moles of Cs are contained in 595 kg of Cs |
4.48 × 10^3 moles Cs |
|
How many moles of potassium are contained in 449 g of potassium? |
11.5 moles |
|
How many Li atoms are contained in 97.9 g of Li? |
8.49 × 10^24 Li atoms |
|
How many iron atoms are contained in 354 g of iron? |
3.82 × 10^24 Fe atoms |
|
How many phosphorus atoms are contained in 158 kg of phosphorus? |
3.07 × 10^27 phosphorus atoms |
|
Calculate the mass (in g) of 1.9 x 1024 atoms of Pb. |
6.5 × 10^2 g |
|
Calculate the mass (in kg) of 4.87 x 1025 atoms of Zn. |
5.29 kg |
|
Calculate the mass (in ng) of 2.33 x 1020 atoms of oxygen. |
6.19 × 10^6 ng |
|
Which of the following is an example of the law of multiple proportions? |
Two different compounds formed from carbon and oxygen have the following mass ratios: 1.33 g O: 1 g C and 2.66 g O: 1 g C. |
|
Which of the following statements is FALSE? |
The halogens tend to form 1+ ions. |
|
Which of the following statements about isotopes is TRUE? |
Some elements have 3 or more naturally occurring isotopes. |
|
Which of the following statements is FALSE? |
The alkali metals are fairly unreactive. |
|
Which of the following doesn’t describe a metal? |
Tend to gain electrons |
|
Which of the following does NOT describe a nonmetal? |
Nonmetals are generally unreactive. |
|
Which of the following statements is FALSE according to Dalton’s Atomic Theory? |
An atom of nitrogen can be broken down into smaller particles that will still have the unique properties of nitrogen |
|
Which of the following statements about subatomic particles is TRUE? |
A neutral atom contains the same number of protons and electrons |
|
Which of the following contains the MOST atoms? You shouldn’t need to do a calculation here. |
10.0 g He |
|
Which of the following contains the FEWEST atoms? You shouldn’t need to do a calculation here |
4.0 g Rb |
|
Why do the isotopes of the same element have the same atomic size? |
Isotopes only differ in the number of protons contained within the nucleus. Since the size of an atom is determined by the electrons, isotopes of the same element should be the same size. |
|
Why doesn’t a mass spectrum of silver have a peak at 107.9 amu? |
The average atomic mass of silver is 107.9 amu, but there are no atoms of silver that weigh 107.9 amu. One isotope weighs more and another weighs less. |
|
Describe an atom and what it is made up of according to modern atomic theory. |
An atom is made up of a nucleus surrounded by electrons. The nucleus contains protons (positively charged particles) and neutrons (neutral particles) and is where most of the mass of an atom comes from, but is a tiny fraction of an atoms volume. The nucleus is surrounded by negatively charged electrons, the same number as there are protons in the nucleus. An atom is therefore neutral overall. |
|
Are anions typically larger or smaller than their corresponding atom? Why? |
Anions are larger than their corresponding atom because the anion contains more electrons than the atom. Since electrons repel one another AND determine the size of the atom or ion, adding electrons to the atom to form an anion makes it larger. |
|
Why do elements in the same group tend to have similar chemical properties? |
Since elements in the same group have the same number of valence electrons (similar electron configurations) they tend to have similar chemical reactivity, since chemical reactions typically involve valence electrons. |
|
magnesium |
Mg |
|
carbon |
C |
|
potassium |
K |
|
iron |
Fe |
|
silicon |
Si |
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