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214 Cards in this Set
- Front
- Back
How many significant figures are in the number 6.022 x 10^23? |
4 |
|
In the product 1.04 x 0.31, the number of significant figures is |
2 |
|
How many significant figures are in the number 60.02 x 10^5? |
4 |
|
How many significant figures are in the number 0.020300? |
5 |
|
Using the rules of significant figures, calculate the following: 12.67 + 13.005 = |
25.68 |
|
If 1.000 kg equals 2.205 lb, what is the mass in pounds of a human who weighs 75.00 kg? |
165.4 lbs |
|
Convert 17.6 cm to inches (2.54 cm = 1 in) |
6.93 |
|
Convert 692 m to decimeters. |
6920 dm |
|
The number of milligrams in 100 g is: |
1 x 10^5 mg |
|
Convert 258 L to milliliters. |
2.58 x 10^5 mL |
|
Correctly rounded, the result of (23.1000 g - 22.0000 g) /(25.10 mL - 25.00 mL) is |
11.0 g/mL |
|
The number 2.00152 rounded to four significant figures is: |
2.002 |
|
In the product 1.04 x 0.31, the number of significant figures is: |
2 |
|
When the calculation (32.8070 × 1.0200) x 0.000201 is carried out, the number of significant figures in the answer is: |
3 |
|
What is the result of this calculation expressed to the correct number of significant digits? (42.785 - 41.808) / 25.56 |
0.0382 |
|
When the calculation (4.60 × 9.315) - 1.0 × 10^2 is carried out, the number of significant figures in the answer is: |
3 |
|
What is the result of this calculation expressed to the correct number of significant digits? 72.1 + 1.684 = ? |
73.8 |
|
Convert 6.0 kg to pounds (1 kg = 2.205 lb). |
13 lb |
|
How many milliliters are in 0.0020 L? |
2.0 mL |
|
The fundamental unit of mass in the metric system is the: |
Gram |
|
The answer that should be reported for the total number of milliliters of solution when 19.10 mL of ethanol is added to 1.52 L of methanol is: |
1.54 x 10^3 mL. |
|
Convert 9.83 kg to pounds (1 lb = 453.6 g). |
21.7 lb |
|
The measurements of three different masses on three different balances are 1.21 kg, 536 mg, and 23.14 g. The total mass should be reported as: |
1.23 x 10^3 g. |
|
A cubic centimeter (cm3) is equivalent to what other metric volume unit? |
mL |
|
The measurement 4.3 x 10^3 g also could be written as ______ kg: |
4.3 kg |
|
The density of copper metal is 8.9 g/mL. What is the mass of 1.00 L of this metal? |
8.9 x 10^3 g |
|
If a 100.-g sample of platinum metal has a volume of 4.67 mL, what is the density of platinum in g/cm3? |
21.4 g/cm3 |
|
The density of copper metal is 8.9 g/mL. What is the volume of 55.0 mg of this metal? |
0.0062 cm3 |
|
The density of an object that has a mass of 2.50 g and occupies a volume of 1.20 cm3 equals: |
2.08 g/cm3 |
|
The density of lead metal is 11.3 g/cm3. What is the volume of 15.0 g of this metal? |
1.33 cm3 |
|
What is the mass of a substance that has a volume of 16.0 mL. The density of this substance is 8.50 g/mL. |
136.0 g |
|
The density of alcohol is 0.780 g/mL. What is the mass of 20.0 mL of the alcohol? |
15.6 g |
|
What is the volume occupied by 56.0 g of a substance, which has a density of 0.940 g/mL? |
59.6 mL |
|
If 1 mi = 1.61 km, what is a speed of 1.0 km/min in mi/hr? |
37 mi/hr |
|
The recommended daily allowance (RDA) of calcium is 1200 mg. Calcium carbonate contains 12 % calcium by mass. How many grams of calcium carbonate are needed to provide the RDA of calcium? |
10.0 g |
|
If a person can comfortably carry 20 kg (44 lbs) and gold has a density of 19.6 g/cm3, what is the volume of the largest piece of solid gold a person can carry? |
1020 cm3 |
|
A car averages 35 miles per gallon of gasoline. How many liters of gasoline will be needed for a trip of 450 km? Some conversion factors which may be helpful are the following: |
3.0 x 10^1 L |
|
A sample of milk is found to have arsenic at a concentration of 1.31 μg/L (microgram/liter). What is the concentration in ounces per gallon? |
1.7 x 10^7 oz/gal |
|
Two types of pure substances are: |
Compounds and elements. |
|
Ice floating in soda water is classified as: |
A heterogenous mixture. |
|
Which property of a sample of a substance would not be characteristic of the substance and hence would not be useful in identifying the substance? |
Mass of the sample. |
|
Gasoline is classified as: |
A homogenous mixture. |
|
In a chemical change, the products: |
are different substances from the starting materials. |
|
Water is an example of:
|
A compound. |
|
If a solution of silver perchlorate is added to a solution of sodium iodide, solid silver iodide forms. The silver iodide is called a:
|
precipitate.
|
|
Muddy water is placed on a porous surface and clear water allowed to seep through. This process is called:
|
Filtration |
|
A pure substance made up of more than one kind of atom is called:
|
An element |
|
The fact that gold does not rust is a: PHYSICAL or CHEMICAL property? |
Chemical property |
|
275°F is equivalent to _________ C? |
135°C |
|
The temperature of a liquid is 247 K. The temperature in ºC would be: |
-26 |
|
423 K equals ______ ºC? |
150.°C |
|
507.1 K is equal to ______ ºF. |
453.4 |
|
22.4 ºC is equal to ______ ºF. |
72.3 |
|
-105 oC is equal to ______ K. |
168 |
|
-53.6 oC is equal to ______ oF. |
-64.5 |
|
What is the change in temperature of 25.0 g of silver (specific heat = 0.240 J/g ºC) if 85.0 J of heat is added to the silver sample? |
14.2 C |
|
How much heat energy is needed to warm 50.0 g of carbon (specific heat = 0.71 J/g ºC) from 25 ºC to 75 ºC ? |
|
|
Heat is typically measured in: |
Joules |
|
How many kilojoules are there in 15.4 kilocalories? |
64.4 kJ |
|
What is the mass of a copper sample (specific heat = 0.384 J/gºC) if addition of 30.0 J of heat causes the temperature to change from 15.2ºC to 35.0ºC |
3.95 g |
|
Which of the following is a valid unit for specific heat (or specific heat capacity)? |
cal/g °C |
|
If 85.1 cal of heat are added to 10.0 g of water (specific heat = 4.184 J/g oC) at 30.0 oC, what is the final temperature of the water sample? |
38.5 ºC |
|
A 6.75-g sample of gold (specific heat capacity = 0.130 J/g °C) is heated using 50.6 J of energy. If the original temperature of the gold is 25.0°C, what is its final temperature? |
82.7 C |
|
How many kilojoules are there in 3.37 X 10^4 calories? |
141 kJ |
|
How many calories are there in 57.0 joules of energy? |
13.6 cal |
|
The quantity of heat required to change the temperature of 1 g of a substance by 1°C is defined as: |
Specific heat capacity |
|
A 13.1 g sample of a liquid changes from 35.0 ºC to 25.0ºC upon removal of 85.0 J of heat. What is the specific heat of this liquid in J/gºC? |
0.649 |
|
An atom that has the same number of neutrons as 59Co has ____ neutrons. |
59 |
|
The mass number of any atom is equal to its: |
number of protons plus neutrons |
|
The first scientist to show that atoms emit tiny negative particles was: |
JJ Thompson |
|
Which atomic particle determines the chemical behavior of an atom? |
Electron |
|
How many atoms of hydrogen are in one molecule of Ca(OH)2? |
2 |
|
The atom with 68 neutrons and 50 protons has a mass number of: |
118 |
|
Common table salt is sodium chloride. When table salt is dissolved in water, the solution conducts electricity because: |
There are ions in the solution |
|
What is the name of the element in Group IIA and period 3 in the periodic table? |
Magnesium |
|
An atom with 45 protons has a mass number of 100. It must contain how many neutrons? |
55 |
|
In the atomic symbol 31P 3-, how many electrons are represented? |
18 |
|
How many protons, electrons, and neutrons, respectively, does O have? |
8, 8, 8 |
|
An atom with 15 protons and 16 neutrons is an atom of: |
P - Phosphorus |
|
Which subatomic particles must always be of equal numbers in any atom? |
Electrons and protons |
|
Atoms of the same element that have different masses are called: |
Isotopes |
|
How many phosphorus atoms are represented by one formula unit of calcium phosphate, Ca3(PO4)2? |
2 |
|
How many electrons are present in a bromine atom with a mass number of 87? |
35 |
|
What is the name of the Group IA metals? |
Alkali metals |
|
An element's most stable ion forms an ionic compound with chlorine having the formula XCl2. If the ion of element X has a mass of 89 and 36 electrons, what is the identity of the element, and how many neutrons does it have? |
Sr, 51 neutrons |
|
What is the symbol of the ion having 12 protons and 10 electrons? |
Mg2+ |
|
Which parts of the atom have approximately the same mass? |
Proton and nutron. |
|
Which particle has the least mass? Proton or electron. |
Electron (mass is negligible) |
|
35.0 pounds of U.S. nickels contain 8.8 pounds of copper. What is the percentage copper in these coins? |
25% |
|
At PCC the student body is 56.3% female. If there are 39 students, on average, in each class at PCC, approximate how many women are there in each class? |
22 |
|
An alloy is made by mixing 40.0 grams of tin, 35.6 grams of lead, and 50.0 grams of copper. What is the percentage of lead in this alloy? |
28.3 |
|
If Sterling silver is 90.0% silver and 10.0% copper, what is the maximum amount of Sterling silver that can be made if you have 49.7 grams of silver metal and an unlimited amount of copper? |
55.2
|
|
It is well known that the element magnesium has three naturally occurring isotopes. Mg-24 represents 79.0% of all magnesium atoms, Mg-25 accounts for 10.0%, and Mg-26 is the remaining 11.0%. If you have 226. atoms of magnesium, how many should be Mg-24?
|
179 |
|
It is generally recognized that a "balanced" diet should contain 30.0% fat. If the average individual requires 2388 Calories of energy from the foods ingested each day, how many Calories should come from fat? |
716 |
|
You wish to buy enough honey to fill a 5.35 quart honey jar. At the grocery story you find that honey costs $3.00 per kilogram and it has a density of 1.50 grams per milliliter. How much will it cost in $ to buy enough honey to fill your 5.35 quart jar? (1 qt = 946 mL)
|
22.8
|
|
An iron ore was found to contain 92.0% pyrite (fool's gold). Pyrite has the formula FeS2and is 46.5% iron. How many grams of iron are there in 65.8 grams of iron ore?
|
28.1 |
|
Methane molecules (the overwhelming majority of the molecules in natural gas) are composed of 25.1% hydrogen and 74.9% carbon, by mass. If there is a reaction between 115.1 g of carbon with 28.3 grams of hydrogen, how many grams of methane could be produced?(Give only the numerical value for answer in the box) |
113.0 |
|
How many electrons are in the third principal energy level (n = 3) of one atom of Fe? |
14 |
|
As the principal energy level increases in an atom's orbitals, the average distance of an electron energy level from the nucleus ______________.
|
Increases
|
|
What element has the electron configuration 1s22s22p63p64s23d104p5?
|
Br |
|
Which of the following is a reasonable criticism of the Bohr model of the atom? |
It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen. |
|
The shape of an s orbital is:
|
Spherical |
|
An element which has the similar valence electron configuration as tellurium (Te) is: |
S |
|
Which subshell can hold the greatest number of electrons?
|
4f |
|
The maximum number of electrons that can occupy the 5f orbitals is: |
14 |
|
The number of unpaired electrons in an oxygen atom is: |
2 |
|
The principal quantum number of the valence electrons in an atom of tin (Sn) is:
|
4 |
|
How many d electrons are there in a vanadium atom? |
3 |
|
The maximum number of electrons allowed in the fourth energy level is: |
32 |
|
The number of p orbitals in the fourth principal energy level is: |
3 |
|
The Group 3 (III A) elements through the Group 8 (VIII A) elements form an area of the periodic table where the electron sublevels being filled are: |
P Orbitals |
|
Which of the following properties generally increases as we go from the left to the right of the periodic table? |
Ionization energy |
|
What main group element forms a positive ion having the ground-state electron configuration [Ar]? |
Calcium |
|
Order the elements S, Cl, and F in terms of increasing atomic radii. |
F, Cl, S |
|
What is ionization energy? |
The energy required to remove an electron from an atom. |
|
Which of the following pairs are isoelectronic (same number of electrons)? |
K+ and Ca2+ |
|
What is the formula used to calculate specific heat? |
q = (m) ⋅ (c) ⋅ (Δt) (q) heat added = (m) mass ⋅ (c) specific heat capacity ⋅ (Δt) change in temp. |
|
What is the formula to calculate density? |
d = m / v |
|
What is the formula for calculating mass? |
m = d ⋅ v |
|
What is the formula for calculating volume? |
v = m / d |
|
Atoms get excited and give off _____________ in the form of light as they return back to their ground state. |
Photon energy |
|
If an elemental atom loses 2 electrons, will it have a positive or negative charge? |
Positive |
|
If an elemental atom gains 2 electrons, will it have a positive or negative charge? |
Negative |
|
A _______ consists of atoms of 2 or more different elements bound together my chemical means. |
Compound |
|
A _________ consists of two or more elements or compounds that are physically intermingled. Often retains many properties of its components. |
Heterogenous mixture
|
|
A _______ often retains many properties of its components. |
Mixture |
|
A _______ often takes on properties different than its component elements. |
Compound |
|
A ________ is a mixture of two or more substances (solute and solvent). |
Solution |
|
A compound can me physically separated: True or False? |
False |
|
Name 5 examples of heterogenous mixtures: |
1.) sandy water 2.) cereal in milk 3.) ice in soda water 4.) oil and water 5.) chicken noodle soup |
|
Name 5 examples of homogenous mixtures: |
1.) gasoline 2.) air 3.) blood 4.) brass 5.) cough medicine |
|
Name 5 physical properties: |
1.) physical state (s,l,g) 2.) color 3.) smell 4.) solubility 5.) melting / boiling points 6.) conductivity 7.) hardness |
|
Name 5 chemical properties: |
1.) corroding 2.) reacting 3.) tarnishing 4.) decomposing 5.) fermentation |
|
℃ to ℉ conversion equation |
℉ = 1.8 (℃) + 32 |
|
℉ to ℃ conversion equation |
℃ = (℉ - 32) / 1.8 |
|
℃ to K conversion equation |
K = ℃ + 273.15 |
|
K to ℃ conversion equation |
℃ = K - 273.15 |
|
1 calorie = __________ joules |
4.184 |
|
What is the specific heat measurement of water? |
4.184 |
|
How many electrons are present in a Fe 3+ atom? |
23 e- |
|
How many "f" orbitals are present in the third energy level? |
None |
|
What is the maximum amount of electrons in an "s" orbital? |
2 |
|
What is the maximum amount of electrons in a "p" orbital? |
6 |
|
What is the maximum amount of electrons in a "d" orbital? |
10 |
|
What is the maximum amount of electrons in a "f" orbital? |
14 |
|
A sample of pure iron requires 142 cal of energy to raise itstemperature from 23ºC to 92ºC. What is the mass of the sample?(The specific heat capacity of iron is 0.45 J/gºC.) |
19? |
|
7 Diatomic Elements: |
Hydrogen H2 Nitrogen N2 Oxygen O2 Fluorine F2 Chlorine Cl2 Bromine Br2 Iodine I2 |
|
Define wavelength: |
the distance between two peaks in a wave |
|
Define frequency (v): |
the number of waves (cycles) per second that pass a given point |
|
Define speed (c): |
the speed of light (2.9979×108 m/s) |
|
In a chemical reaction, matter is: |
Neither created or destroyed. |
|
Energy is: |
the capacity to do work |
|
Work is defined as: |
the result of force acting on a distance |
|
The behavior of matter is driven by: |
Energy |
|
The energy needed to raise the temperature of 1 gram of water through 1 °C (now usually defined as 4.1868 joules). |
1 calorie |
|
1 calorie equals ________ joules. |
4.184 |
|
1 Cal = ______ cal |
1000 |
|
1 kcal = _______ cal |
1000 |
|
1 Calorie equals ________ joules. |
4184 |
|
60.1 cal to joules |
251j |
|
105.8 F = ________ C |
41 C |
|
37 C = _________ K |
310.15 K |
|
JJ Thompson |
Credited with the discovery and identification of the electron; and with the discovery of the first subatomic particle. He proposed that atoms must contain positive charge that balanced the negative charge of electrons. |
|
Dalton's Atomic Theory |
1) All matter is made of atoms. Atoms are indivisible and indestructible. 2) All atoms of a given element are identical in mass and properties 3) Compounds are formed by a combination of two or more different kinds of atoms. 4) A chemical reaction is a rearrangement of atoms. |
|
Bohr Atomic Model
|
Depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus—similar in structure to the solar system, but with attraction provided by electrostatic forces rather than gravity.
|
|
Rutherford Atomic Model |
Correctly explained nuclear atom: nucleus, protons (+) and electrons (-). |
|
Name group 1A: |
Alkali Metals |
|
Name group 2A: |
Alkaline Earth Metals |
|
List the 7 metalloids: |
B Si Ge As Sb Te At |
|
Name group 7A: |
Halogens |
|
Name group 8A: |
Noble gasses |
|
Most reactive group (1A-8A): |
1A |
|
Least reactive group (1A-8A): |
8A |
|
Positive ions are called: |
Cations |
|
Negative Ions are called: |
Anions |
|
If an atom loses a(n) electron(s), its charge becomes: |
Positive |
|
If an atom gains a(n) electron(s), its charge becomes: |
Negative |
|
An ______ chemical element is an atom that has a different number of neutrons (that is, a greater or lesser atomic mass) than the standard for that element. |
Isotope |
|
Calculate the atomic mass of Ga: Ga-69 (60.11% mass 68.9256 amu) Ga- 71 (39.89% mass 70.9247 amu) |
69.72 amu |
|
A _________ is a statement based on repeated experimental observations that describes some aspects of the universe. |
Scientific law |
|
A _______ always applies under the same conditions, and implies that there is a causal relationship involving its elements. |
Scientific law |
|
A __________ is a well-substantiated explanation of some aspect of the natural world, based on a body of facts that have been repeatedly confirmed through observation and experiment. Such |
Scientific theory |
|
Fact-supported ________ are not "guesses" but reliable accounts of the real world. |
Scientific theories |
|
________ is the active acquisition of information from a primary source. |
Observation |
|
In living beings, _________ employs the senses. |
Observation |
|
In science, ________ involves the recording of data via the use of instruments. The term may also refer to any data collected during the scientific activity. |
Scientific observation |
|
The _________ is the energy carried by a single photon with a certain electromagnetic wavelength and frequency.
|
Photon energy
|
|
The higher the photon's ________, the higher its energy. |
Frequency |
|
How many significant figures are counted when multiplying or dividing? |
The least amount of figures used in the initial equation. |
|
How many decimals are counted when adding or subtracting? |
The least amount of decimals used in the initial equation. |
|
Convert a 10 cm x 12 cm x 15 cm box to cubic inches. |
109.8 in3 |
|
How many cubic inches is in 3.25 yard 3? |
|
|
If 75.0 g of copper is added to 50.0 mL of water in a graduated cylinder and the water lever rose to 58.4 mL, what is the density of the copper |
8.4 cm3 |
|
What is the mass in grams of a cube of gold (density= 19.32 g/cm3) if the length of the cube is 2 feet. |
|
|
A ________ has definite volume and maintains its shape. |
Solid |
|
Particles vibrate and oscillate but to not change position. |
Solid state |
|
A _______ has definite volume but no definite shape. |
Liquid |
|
A ______ assumes the shape of its container |
Liquid |
|
A _______ has no fixed volume or shape. |
Gas |
|
A _______ takes the shape and volume of its container and are compressible. |
Gas |
|
Two types of pure substances: |
Elements and compounds |
|
A _________ is formed when two or more atoms join together chemically. |
molecule |
|
Define molecule: |
A molecule is formed when two or more atoms join together chemically. |
|
Define pure substance: |
Composed of only 1 type of atom or molecule. |
|
A ___________ is a molecule that contains at least two different elements. |
Compound |
|
All __________ are molecules but not all molecules are _________. |
Compounds |
|
All compounds are __________ but not all _________ are compounds. |
Molucules |
|
A ______ is a substance composed of a given combination of elements, that can be broken down into individual elements by chemical methods. |
Compound |
|
Define compound: |
A substance composed of a given combination of elements, that can be broken down into individual elements by chemical methods. |
|
The H atom has a volume in approximately 6.2 x 10 -31 m3. What is its volume in nm3? |
|
|
Cu-63 (69.17% at 62.93 amu) Cu-65 (30.83% at 64.93 amu) |
62.55 amu |
|
The greater the energy, the larger the _________. |
Frequency |
|
The higher the frequency, the shorter the __________. |
Wavelength |
|
The higher the energy, the shorter the ___________. |
Wavelength |