Chemistry
Formula to determine percent composition by mass (where E is any element)
% E= (mass of E/mass of sample) x 100%
Method for determining the number of moles of SO3 that will form from the complete reaction of 1.5 mol of O2 2S(s) + 3O2 (g) -> 2SO3 (g)
(1.5 x 2) / 3
What is the oxidation number of boron in sodium tetraborate, Na₂B₄O₇?
+3
A 1.6 g piece of iron was placed in a calorimeter containing 250g of water. The temperature of the water was seen to decrease from 26.5°C to 22.1°C. Calculate the heat change for the metal.
+4.6 kJ
Calorie
- 1 calorie = 4.184 joules - the amount of heat needed to raise the temperature of 1 g of water by 1 degrees celcius.
Statements that correctly describe the information conveyed by the balanced chemical equation: 16Cu(s) + S8(g) -> 8Cu2S (s)
- 16 atoms of Cu react with 1 molecule of S8 to form 8 formula units of Cu2S - Cu and S8 are reactants and Cu2S is the product - 16 molecules of Cu react with 1 mole of S8 to form 8 moles of Cu2S
Correctly describe the information conveyed by the following balanced chemical formula: 16Cu(s) + S₈(g) -> 8Cu₂S(s)
- 16 atoms of Cu react with 1 molecule of S₈ to form 8 units of Cu₂S -Cu and S₈ are reactants and Cu₂S is the product - 16 moles of Cu react with 1 mole of S₈ to form 8 moles of Cu₂S
Display the relationship between 1mg and 1g
- 1g/10^3mg - 10^-3g/1mg
Metric Conversion examples
- 1kg/10^3g - 1ng/10^-9g
Combinatorial Chemistry
- A series of related chemical compounds is systematically prepared and tested for effectiveness
Hypothesis
- A tentative explanation for the properties or behavior of matter that accounts for a set of observations
Formula for compound containing the silver ion and the carbonate ion:
- Ag2CO3
compounds containing polyatomic ions
- Al(NO3)3 - NH4F - BaCO3
Scientific Method
- An approach to asking questions and seeking answers that employs a variety of tools, techniques, and strategies
Quantitative Observation
- An observation based on numerical value
Qualitative observation
- An observation based on some quality of matter
Polyatomic ions are ions that contain two or more______
- Atoms
A gold atom with 79 protons and 76 electrons is a:
- Cation
Consider the following balanced chemical equation: 2Al(s) + 3Cl₂(g) → 2AlCl₃(s) Suppose that eight atoms of Al(s) are reacted with nine molecules of Cl₂(g).
- Cl₂(g) is the limiting reactant - six formula units of AlCl₃ will be formed
Which metals can exhibit multiple charges?
- Cobalt, iron
ZnCO3
- Contains a metal cation with a polyatomic anion
(NH4)2S
- Contains a polyatomic cation with a monatomic anion
(NH4)3PO4
- Contains a polyatomic cation with a polyatomic anion
Characteristics of a molecular compound
- Create nonelectrolyte solutions - Contain only nonmetals
Metals which can form a cation with multiple charges
- Cu - Mn
Which statements correctly describe the features of the periodic table: - Each column in the periodic table is called a group or family of elements -The Periodic table is used by chemists to classify mixtures. - The elements in each column of the periodic table share similar properties - The elements in each row of the periodic table share similar properties
- Each column in the periodic table is called a group or family of elements - The elements in each column of the periodic table share similar properties
Law of conservation of Energy
- Energy cannot be created or destroyed - Energy can be converted from one form into another
CH3CH2OH
- Ethanol - nonelectrolyte - Molecular compound ( non-electrolyte or weak electrolytes)
Theory
- Explains why observations, hypotheses, or laws apply under many different circumstances
Which of the following formulas for a compound containing Fe³+ ion is incorrect? FeS FePO4 Fe2S3 FeBr3 FeN
- FeS
To achieve the stability of a noble gas, elements in group VIIA ________ an electron to be like the closest noble gas
- Gain
products from the reaction between aqueous sodium hydroxide, NaOH, and sulfuric acid H2SO4
- H2O (I) - Na2SO4 (aq)
Acid compounds
- HF - HCN
The name of the group of elements found on the far right of the periodic table that forms ions with 1- charge is the ______
- Halogens
Ionic compounds
- High boiling point due to the strong charge-charge interactions between the ions
What is the name of the acid containing only hydrogen and bromide?
- Hydrobromic acid
Ionic solids contain densely packed _____
- Ions of alternating positive and negative charge
Percent composition by mass
- It is constant no matter what the size of the sample - It is the ratio of the mass of an element to the mass of the sample, multiplied by 100.
N2O4
- Low boiling point - Molecular compound
Nonelectrolyte solutions contain ______ compounds. These compounds _______ dissociate into ions when dissolved in water.
- Molecular, WIll not
What are common compounds that are bases when dissolved in water?
- NH3 - Ca(OH)2 - NaOH
Which of the following is not an example of a physical property? - Nitrogen is colorless - Nitrogen is a gas at room temperature - Nitrogen gas is less dense than oxygen gas - The boiling point of liquid nitrogen is 77 K - Nitrogen combines with oxygen in an internal combustion engine to form oxides of nitrogen
- Nitrogen combines with oxygen in an internal combustion engine to form oxides of nitrogen
Monoatomic anions
- O2- - Cl-
Information given in the formula C5O2
- One molecule of the compound contains two oxygen atoms - One molecule of the compound contains five carbon atoms
Which of these molecules or ions has a violation of the octet rule (other than H)?
- PCI5
A base is a substance that _______
- Reacts with acid to produce water
Information about a binary compound contained in its formula:
- SUbscripts that show the number of the atoms of each element present - The symbol for each element in the compound
NaBr
- Sodium bromide - Contains a monatomic anion and cation
Statements which correctly interpret the following balanced chemical equation: 4HCI(aq) + MnO₂(s) → MnCl₂(aq) + 2H₂O(g) + Cl₂(g)
- The MnCl₂ is dissolved in water - HCI is a reactant in this equation
Law
- The behavior of matter that is so consistent that it appears to have universal validity
Energy
- The capacity to do work or to transfer heat
General characteristic of an ionic compound:
- The compound contains metals and nonmetals - The compound contains anions and cations - The compound has an overall charge of 0
Green Chemistry
- The development of chemical processes that prevent pollution and reduce the amount of natural resources used to manufacture various consumer, research, and industrial products
Kinetic Energy
- The energy of motion
Potential Energy
- The energy possessed by an object because of its position or state
statements on balancing of chemical equations
- The last atoms to balance in an equation are the elemental substances, such as O2 - equation shows the identities and physical states of the reactants and products together with their relative qualities
Steps performed to convert grams of x to grams of y for the following genric reaction: X + A -> 2Y + B
- The number of moles of y is converted into the mass of y using the molar mass of y - The mass of X is converted into moles of X using the molar mass X - The number of moles of X is converted into the mass number of moles of y using the molar ratio of x and y
Why do ionic compounds form brittle, harb solids that melt at very high temperature ?
- The oppositely charged anions and cations attract each other tightly in the solids - The ions form and ordered crystal lattice
Statements about naming a molecular compound like C3O2
- The prefix tri- would be written before the word carbon - The second element would be named with a greek prefix followed by -oxide
Information gained from a balanced chemical equation
- The relative quantities (moles) of a substance involved - The identities of substances involved - The physical states of reactants and products often , but not always
A formula unit is _______
- The smallest repeating unit in an ionic crystal lattice
The compound BaI2, is water soluble. When a small amount of solid BaI2 is placed in water and stirred carefully, what happens?
- The solid BaI2 no longer appears visible to the naked eye - The BaI2 releases Ba3+ and I- ions
Ration of calcium to chloride ions in the ionic compound calcium chloride (CaCl2)
- There is one calcium ion (Ca2+) for every two chloride ions (Cl-) in calcium chloride
Physical properties of ionic solids
- They are brittle solids - They are solids at room temperature
Properties of ionic solids
- They are solid at room temperature - They are brittle solids
Total number of ions in the compound Mg(OH)2
- Three ions
The formula for a compound containing sodium and oxide ions would contain _____. This compound would have an overall ______ charge.
- Two sodium and one oxide ion; neutral
Describe volume:
- Volume is a three-dimensional quantity - Volume is the amount of space a substance occupies - The volume of a cube is equal to the length x width x height
Molarity (M) true statements
- When adding water to a solution, the moles of solute stay constant - Increasing the volume of a solution by adding more water decreases the molarity
The compound KBr is an electrolyte. This compound :
- Will dissolve in water to produce K+ and Br- ions - Produces a solution that will complete a circuit and light a bulb
Line Spectra
- a line spectrum provides that the electron structure of the atom is quantized. -a line spectrum results when an element is heated or given an electric charge and the energy absorbed is transferred into light energy
statements describing a combustion reaction
- a reaction that involves oxygen molecules as reactants - a reaction that rapidly produces heat and flame
Which of the following are homogeneous mixtures? - a jar of chunky salsa - pure water containing no additional compounds - a red sports drink containing sugar, salt, and food coloring - a well-mixed sample of sugar water
- a red sports drink containing sugar, salt, and food coloring - a well-mixed sample of sugar water
Orbitals
- a region of space in which an electron is likely to be found
Neutralization reactants
- are double-displacement reactions - occur between an acid and a base
Electromagnetic radiation
- consists of oscillating electric and magnetic fields - energy in the form of light is called electromagnetic radiation - travels through space as oscillating waves
4p
- each orbital represented is of the same shape and energy - the principle energy level is equal to 4 - the letter p represents orbitals px, py, and pz
Valence electrons of elements
- for any main group element the number of valence electrons is equal to the number of electrons in the highest-energy s and p sublevels - main-group elements in the same group of the periodic table have the same number of valence electrons - the valence electrons of an atom reside in the same principle energy level, n.
Possible driving forces for a double displacement reaction
- formation of a gas - formation of a precipitate (in insoluble solid) - formation of water or other molecular compound
(NH4)2CO3
- high melting point - ionic compound (ammonium and carbonate ions)
Which of the following is not an example of matter? - wax - air - a stain on clothing - the propellant in an aerosol can - light from a candle
- light from a candle
Molecular compounds
- low boiling point due to the weak interaction between molecules in their liquids
Items required when writing a chemical equation
- product symbols - phase labels - reactant symbols
Describe a Empirical formula
- simplest ratio of elements in a compound - written with the smallest whole-number subscripts - usually the way that the ionic compound are represented
NaCl
- strong electrolyte - ionic compound (most common ionic compounds are strong electrolytes)
Which of the following is not a chemical property? - sugar will dissolve in water - a steak on a hot frying pan will turn brown - water can be decomposed to hydrogen and oxygen - gasoline will burn if ignited - An iron nail will rust in water
- sugar will dissolve in water
Frequency
- symbolized by the greek letter nu, ν - described in units of 1/2, s−¹, or hertz (Hz) - a measure of the number of wave cycles that move through a point in space in 1 second
Actual yield of a chemical reaction
- the amount of product obtained in the lab from a chemical reaction - amount of product that is measured to have formed from a chemical reaction
Which of the following statements is incorrect? - evaporation of water from a fish tank is evidence of a physical change - the burning of a piece of charcoal to a white powder is an example of a physical change - The fact that copper conducts electricity is a physical property - The condensation of steam on a mirror is an example of a physical change.
- the burning of a piece of charcoal to a white powder is an example of a physical change
Chemical Properties can be defined by:
- the composition of a substance - what chemical changes it
Principle energy level
- the larger the numerical value of the principle energy level (n), the larger the orbital size - the principle energy level(n) is represented with a positive integer
Limiting reactant in a solution
- the maximum amount of product formed is the amount that can be formed from the limiting reactant - the limiting reactant limits the amount of product(s) that can be formed - When two reactants are mixed together and are not present in the exact mole ratio, we will have too much of one reactant and not enough of another
statement about chemical activity series
- the most active elements appear at the top
Percent yield
- the obtained yield in comparison to the maximum yield that may be obtained from a chemical reaction
Describe a system and its surroundings.
- the surroundings are everything that surrounds a system - Heat absorbed by a system comes from its surroundings
Electron configuration: 1s²2s²2p⁴
- this represents a ground state electron configuration - 8 total orbitals are represented
A 5.2 g piece of metal is heated and placed in calorimeter that is filled with 120g of water that is at 23.5°C. The water reached a final temperature of 74.3°C. Calculate the heat change for the piece of metal (the specific heat of water is 4.184 J/g°C
-25.5 kJ
A 102.0 g sample of water is cooled from 25 ° C to 16.7 ° C. Given the specific heat of water is 4.184 J (g °C), calculate the value of q for this process.
-3.8 kj
Calculate the freezing point of 1.0 m solution of Ca(NO₃)₂ in water. Remember that Mg(NO₃)₂ is an electrolyte. The normal freezing point of pure water is 0.00°C. Kf(water)= -1.86°C/mol
-5.58 ° C
Electromagnetic spectrum
-the visible region of the electromagnetic spectrum includes light we see with our eyes, and represents wavelengths from 400 nm to 750 nm - electromagnetic radiation can be classified according to type if the wavelength of the frequency of the light is known - includes all types of electromagnetic radiation
Observations that indicate a chemical reaction has taken place
-two clear, colorless liquids are added together, and the resulting solution becomes warm - two clear, colorless liquids are poured together, and the resulting solution turns red
45.5 mL sample of a 0.155 M NaCl stock solution is diluted to a final volume of 250.0 mL. Find the concentration (M) of the new solution.
0.0282 M
How many moles of calcium carbonate (CaCO₃, 100.9 g/mol) are there in 6.15 g of calcium carbonate?
0.0614 moles
Consider the following reaction and the value of its equilibrium constant: FeO(s) + CO(g) ⇌ Fe(s) + CO₂(g) Keq=0.67 if the equilibrium concentration of CO is measured at 0.15 M, What is the equilibrium concentration of CO₂?
0.10 M
How many moles of NaCl are contained in 50.0 mL of 2.50 M NaCl?
0.125 moles
Calculate the number of moles and the mass of gas in 3.40 L of He at STP
0.152 mol, 0.608 g
Calculate the number of moles of CaCO₃ (calcium carbonate, or limestone) in a 20.0 g sample of this substance.
0.200 mole
A can of cashews has a mass of 8.5 ounces? what is this mass in Kg? (16 ounces = 453.6g)
0.24 kg
What volume of 2.00 M HCl contains 0.50 mol HCl?
0.25 L
Calculate the number of moles of NaOH (Sodium hydroxide, an ingredient in drain cleaners and oven cleaners) in a 10.0 g sample of this substance.
0.250 mole
How many moles of NaOh are contained in 100.0 mL of 3.00 M NaOH?
0.300 moles
Find the mass (in grams) of LIF present in 45.0 mL of 0.337 M Lif solution. The molar mass of Lif is 25.94 g/mol
0.393 grams
What volume of 6.00 M NaOH contains 2.50 mol NaOH?
0.417 L
How many moles of aluminum bromide (AlBr₃, 266.68 g/mol) are present in 137 g of aluminum bromide?
0.514 mol
When a 25.00 mL sample of NaOH is titrated with 0.2523 M H₂SO₄. 26.29 mL of H₂SO₄ solution is required to neutralized the NaOH. What is the molarity of NaOH?
0.5387
What volume of 3.00 M NaOH contains 1.75 mol NaOH?
0.583 L
A loaf of bread has a mass of 24 ounces. What is the mass in kg? (16 ounces =453.6 g)
0.68 kg
Calculate the density of Ne in g/L at 22.0°C and 735 torr
0.806 g/L
24 kj of energy is required to heat a 250-g sample of aluminum from 10 ° C to 117 °C. what is the specific heat of aluminum.
0.90 J/( g ° C)
Ca(HCO3)2
1 C atom/ 1 H atom
The correctly drawn lewis structure for HCN will have _________
1 single bond, 1 triple bond, and 1 pair of nonbonding electrons
Consider the half-reaction ClO-(aq)→ Cl-(aq). When the equation is balanced in basic solution, the coefficient for water will be ______, and the number of electrons transferred will be ________.
1,2
Four substances and their specific heats are listed below. suppose you wish to raise the temperature of 1 g of each substance by 1°C. Rank the substances according to the amount of heat that will be needed (greatest to least)
1. Aluminum 0.895 J/g°C 2. Copper 0.337 J/g°C 3. Iodine 0.214 J/g°C 4. Mercury 0.140 J/g°C
Consider the following generic balanced chemical equation: A → B The process of converting the mass of the reactant (A) into another (B) (mass-mass conversion) involves three basic steps which are:
1. Convert grams of A into moles (using molar mass of A) 2. Convert moles of A into moles of B (using the mole ratio of A and B) 3. Convert moles of B into the mass of B (using molar mass of B)
Steps of writing a formula of an ionic compound if given the number of its components
1. Determine the formula for any polyatomic ion present 2. Determine the charge on the ions that make up the compound. For monoatomic consult the periodic table, for polyatomic ions recall the charge. 3. Write the cation fist in the formula, then the anion 4. Use the charges on the cation and anion to determine the correct subscripts to give a neutrally charged formula unit
Process of naming the compound with the formula Co(CH3CO2)3
1. Identify the cation as cobalt and the anion as acetate 2. Identify the charge of the acetate as -1 3. Write the name of the cation cobalt and determine its charge of 3+ 4. Write the roman numeral III in parenthesis 5. Write the name of the anion acetate
Describe the process of naming an acid that contains a polyatomic ion
1. Identify the polyatomic ion in the acid formula 2. Write the base name of the polyatomic ion 3. Write the suffix -ic if the polyatomic ion ends in -ate or -ous if the polyatomic ion ends in -ite 4. Write the word acid
Steps concerning the development of the scientific knowledge in order in which they occur
1. Obtain data from observations or experiments 2. Recognize patterns or trends 3. Propose and test hypothesis 4. Propose theory
Steps for writing a balanced equation
1. Write the correct formulas for reactants and products, separated by an arrow 2. Add the physical stat symbols for all substances 3. Count the atoms of each element of the reactant side and on the periodic table 4. if the number of atoms of an element are not equivalent on both sides of the reaction, add a coefficient in front of a reactant or product 5. Make a final check of the number of atoms of each element, on each side of the reaction, to make sure they are equal
General process for naming binary molecular compounds when given the formula
1. Write the name of the element that is the farthest to the left and nearest to the left and nearest to the bottom of the periodic table 2. Add a greek prefix that matches the subscript in the formula for the element if there is more than one atom present 3. Write the root name of the second element present 4. Add the -ide to the root name of the element 5. Add a greek prefix that matches the subscript in the formula of the element ending in -ide
Naming acids that do not contain polyatomic ions:
1. Write the prefix hydro- 2. Write the stem name of the non hydrogen element in the acid 3. Write the suffix -ic 4. Add the word acid
Describe the process for naming simple binary compounds by order in steps.
1. identify the cation and anion 2. Write the name of the cation with its element name 3. Write the root of the anions name and add -ide to the root
steps for determining empirical formula
1. obtain moles of each element 2. divide all mole values by the smallest mole value to obtain whole number ratios 3. write the empirical formula for using the whole numbers as subscripts
Which of the following aqueous solution should have the lowest freezing points? 1.0 m C₁₂H₂₂O₁₁ All should have the same freezing point 1.0 m MgCl₂ 1.0 m NaCl 1.0 m NaNO₃
1.0 m MgCl₂
Calculate the H₃O+ concentration in 0.0010 M HCl.
1.0 x 10-³ M
Density of a solution that is made by dissolving 45.5 g of NaNo3 in sufficient water to make 500.0 mL of solution. The molar mass of NaNO is 84.99 g/mol
1.07 M
Molarity for a solution is made by dissolving 45.5g of NaNO3 in sufficient water to make 500.0 mL of a solution. The molar mass of NaNO3 is 84.99g/mol
1.07 M
Consider the following chemical equation: PCI3(l) + 3H2O(l) -> H3PO3(aq) + 3HCI(g) If 3.48 mol of H2O are reacted with 1.30 mol of PCI3, how many mol of H3PO3 will be produced?
1.16 mol
When a 0.525 g piece of zinc is placed in a solution of copper(II) Sulfate, copper metal and zinc sulfate are formed. Balance the equation for the reaction, and determine the mass of copper (II) sulfate that would react with this quantity of zinc. Zn(s) +CuSO₄(aq) -> ZnSO₄(aq) + Cu (s) (unbalanced)
1.28 g
Molecules of C2H4 are present in a 62.5g sample of C2H4? if the molar mass of C2H4 is 28.05 g/mol
1.34 x 10^24 molecules
Given a fixed amount of gas in a rigid container (no change in volume), what will the gas exert if the pressure is initially 1.50 atm at 22.0°C, and the temperature is changed to 11.0°C
1.44 atm
Molarity of a solution that is made by dissolving 28.4g of KCI in water to make 250.0 mL of solution (the molar mass of KCI is 74.55 g/moles)
1.52 M
Calculate the number of moles in 45.0 g of N₂, and the pressure that would exert at 20.0°C in a 5.00 L steel tank
1.61 mol, 7.74 atm
A sample of gas occupies 2.50 L at a pressure of 0.900 at 22.0°. What will the pressure be if the temperature is changed to 56.5°, and the volume is changed to 1.50
1.68 atm
What is the pH of 0.0015 M HNO₃ solution?
1.82
If the initial pressure of a 3.00 L gas sample is 2.50 atm, what will the pressure be if the volume is changed to 4.00 L at constant temperature?
1.88 atm
Solve for the mass of 85.4 kg in units of pounds (1lb=453.6g)
1.88 x 10^2 lb
Number with its greek prefix for this value
10 - Deca- 9 - Nona- 6 - Hexa- 3 - Tri- 2 - Di-
Calculate the boiling point of a 4.0 m solution of sucrose in water. sucrose is a nonelectrolyte. The normal boiling point of pure water is 100°C. Kb(water) =0.52°C/m
102.1 °C
Calculate the boiling point of 4.0 m solution of sucrose. Sucrose is a nonelectrolyte. The normal boiling point of pure water is 100.0°C. Kb(water)=0.52°c/m
102.1°C
When mercury oxide, a red crystalline solid, is heated, it decomposes to form liquid mercury and oxygen gas, according to the following equation: HgO(s) -> Hg(l) + O2 (g) (unbalanced) Balance the equation and determine the mass of mercury that should be formed when 12.3 g of HgO is heated.
11.4g
Calculate the molar mass of C₃H₆Cl₂
112.98 g/mol
Quantities matched with description.
12 - one dozen 2 - one pair 6.022 x 10^23 - one mole
What is the percent-by-mass concentration of KCl In a solution that is prepared by adding 13.0 g of KCl to 85.0 g of water?
13.3%
Potassium chloride is used medically as an electrolyte replenisher. Determine the mass of potassium in a 250-mg tablet of potassium chloride. Potassium chloride is 52.4% potassium by mass.
131 mg
Mass of a 2.16-mol sample of HNO3
136g
Mass of a mole of 2.16 mol sample of HNO3
136g
Consider the following balanced equation: 3H2+N2 -> 2NH3 Calculate the mass of NH3 produced by the complete reaction of 2.55g of H2. The molar mass of NH3 is 17.03 g/mol.
14.4g
The number of neutrons in an atom of uranium is:
143
Propane burns in air according to the equation: C₃H₈(g) + 5O₂(g) -> 3CO₂ + 4H₂O(g) what volume of CO₂ would be formed if 5.00 L of propane burns, assuming that all of the gases are under the same conditions?
15.0 L
List the number of protons, neutrons, and electrons for ³⁵Cl
17 protons, 18 neutrons, and 17 electrons
which of the following is the correct ground state electron configuration for a phosphorus atom?
1S² 2S² 2P⁶ 3S² 3P³
Which of the following is the correct ground state electron configuration for a sulfur atom?
1s² 2s² 2p⁶ 3s² 3p⁴
Which of the following is the correct ground state electron configuration for chlorine?
1s² 2s² 2p⁶ 3s³ 3p⁵
Which of the following is the correct ground state electron configuration for a sulfur atom?
1s²2s²2p⁶3s²sp⁴
How many single bonds are typically formed by the element O
2
Conversion factors that correctly represent the molar relationship in the balanced chemical equation 2Al+3Cl2 -> 2AlCl3
2 mol AlCl3/3 mol Cl2 2 mol Al/3 mol Cl2
Volume (in L) of a 0.225 M MgSO4 solution contains 62.5 grams of MgSO4? The molar mass of MgSO4 is 120.37 g/mol
2.31 L
Consider the following balanced chemical equation: Pb(NO₃)₂(aq) + 2KI(aq) → PbI₂(s) + 2KNO₃(aq) if 1.70 g of Pb(NO₃)₂ are reacted with 3.40 g of KI, how many grams of PbI₂ will be produced? The molar masses of Pb(NO₃)₂, KI, and PbI₂ are 331.22, 166.00 and 461.00 g/mol, respectively.
2.36 g
if the pH of a certain soft drink is 3.60, What is the H₃O+ concentration in the soft drink?
2.5 x 10-⁴ M
Calculate the number of moles in 75.0 g of N₂, and the volume that it would occupy at 50.0°C and 1.50 atm
2.68 mol, 47.4 L
Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 3.50 L sample were cooled from 90.0°C to 30.0°C
2.92 L
A bottle of gatorade has a volume of 591 mL. What is this volume in fluid ounces? (1 fluid ounce=29.57mL)
20.0 Fl oz
A solution of acetic acid, CH₃CO₂H, is prepared by dissolving 30.0 mL of acetic acid in enough water to give a total volume of 150.0 mL. what is the percent-by-volume of acetic acid?
20.0%
The isotope symbol for an ion that has 11 protons , 12 neutrons, an 110 electrons is:
23/11 Na+
Mass of a 3.11 mol sample of CS2
237 grams
The formula for novocaine, a local anesthetic, is C₁₃H₂₁N₂O₂. What is the molar mass of this compound?
237.32 g/mol
Physophine, PH3, a reactive and poisonous compound, reacts with oxygen as follows: 4PH₃(g) 8O₂(g) -> P₄O₁₀(s) + 6H₂O(g) if you need to make 6.5 moles of P₄O₁₀, how many moles of PH₃ is required for the reaction?
26 moles
Balance the following skeletal equation using the fractional coefficients method: KNO3(s) -> KNO2 (s) + O2(g)
2KNO3(s) -> KNO2(s) + O2 (g)
Balance the following skeletal equation: Li(s) + H₂O(l) -> LiOH(aq) + H₂(g)
2Li(s) + 2H₂O(l) -> 2LiOH(aq) + H₂(g)
Which of the following is formed when (NH₄)₂SO₄ dissolves in water?
2NH₄ + SO₄²-
What ions, atoms, or molecules (in addition to the water molecules) are present after Na₂SO₄(s) mixes with water?
2Na+(aq) + SO₄²- (aq)
Decomposition of solid potassium chlorate to form oxygen gas and solid potassium chloride
2kCIO3(s) -> 2KCI (s) + 3O2(g)
The valence level and the number of valence electrons, respectively, for chlorine, are
3 and 7
The element phosphorus will form an ion with a charge of
3- written as: P3-
How many carbon atoms are there in 0.50 mole of CO2?
3.0 x 10²³
Calculate the photon energy (Ephoton) for light with a wavelength of 565 nm
3.52 x 10-¹⁹ J
A solution contains 15.5 g NaOH dissolved in sufficient water to give a total mass of 125.0g. What is the molality of the solution?
3.54 m
A 200.0 g sample of river water contains 6.4 mg of lead. How many parts per million of lead are in the sample?
32 ppm
The number of protons and neutrons in an atom of bromine-81 is:
35 protons and 46 neutrons
Calculate the molar mass of Fe₃(PO₄)₂:
357.49 g/mol
On the planet Melmac, in a galaxy far, far away, argon has three naturally occurring isotopes as follows: Isotope mass (amu) Natural abundance (%) Argon-40 39.962 74.20 Argon-38 37.963 15.15 Argon-36 35.968 10.65 What is the relative atomic mass of argon on Melmac?
39.23 amu
CH4O
4 H atoms/ 1 C atom
The correctly drawn lewis structure for CBr₄ will have _________.
4 single bonds
The correctly drawn lewis structure for SiH₄ will have ___________.
4 single bonds to Si
A laser use in DVD players has a wavelength of 405 nm. What is the energy of this light in joules?
4.91 x 10-¹⁹J
Convert 6.25 x 10⁴ Pa to mm Hg
469 mm Hg
Consider the following balanced chemical equation: 2C₂H₆(g) + 7O₂(g) → 4CO₂(g) + 6H₂O(l) How many moles of O₂ will be required ti react with 14 moles of C₂H₆?
49 moles
Balance the following skeletal equation: NH₃(g) + O₂(g) -> NO₂(g) + H₂O(g)
4NH₃(g) + 7O₂(g) -> 4NO₂(g) + 6H₂O(g)
The wavelength of the yellow light given off by a sodium vapor street lamp is 589 nm. what is the frequency of this light in hertz (S-¹)?
5.09 x 10¹⁴S-¹
The number 54,900 Correctly expressed in scientific notation is:
5.49 x 10⁴
A solution contains 22.0 g of HCl dissolved in sufficient water to give a total mass of 125.0g. What is the molality of the solution?
5.86 m
The solubility of potassium chloride is 34.2 g/100.0 g of water at 20°C. Which of the following best describes a solution prepared by adding 58.3 g of potassium chloride to 150.0 g of water at this temperature?
51.3 g of KCl will dissolve and 7.0 g will remain undissolved
What is the total number of electrons that can occupy a 5p sublevel?
6
C2H6O
6 H atoms/ 2 C atoms
Consider the following balanced chemical equation: CO(g) + 2H₂(g) → CH₃OH(g) if 7 molecules of CO are reacted with 12 molecules of H₂, how many molecules of CH₃OH can be formed?
6 molecules of CH₃OH
Consider the reaction: Zn(s) + NO₃-(aq)→ NH₃(aq) + Zn(OH)₄²-(aq) When this equation is balanced in a basic solution, the coefficient for water will be ________, and the number of electrons transferred will be __________.
6,8
What is the molal concentration of ions in a 1.60 m solution of Fe(NO₃)₃?
6.40 m
The EPA has determined the maximum safe level of lead ion in drinking water is 15 ppb. If a sample of tap water has a lead ion concentration of 0.0065 ppb, what is the concentration of the lead ion in ppb, and is the water safe to drink? Assume the density of the solution is 1.00 g/mL.
6.5 ppb, Safe
The correct answer for the subtraction between 28.645 g -22.105 g is:(considering significant figures)
6.540 g
Percent hydrogen in glucose, if a 8.27g sample of glucose contains 0.555g of hydrogen
6.71%
Given that 4NH₃(g) + 5O₂ -> 4NO(g) +6H₂O, if 4.5 moles of NH₃ react with sufficient oxygen, how many moles of H2O should form?
6.8
Ammonia is usually made by the following reaction. N₂(g) + 3H₂(g) -> 2NH₃. What is the maximum amount of ammonia that can be formed if 30 molecules of nitrogen are mixed with 100 molecules of hydrogen?
60 molecules
What volume of 0.1243 M KOH is required to neutralize 25.00 mL of 0.1540 M H₂SO₄? (First write a balanced equation for the reaction)
61.95 mL
Calculate the amount of heat energy required to evaporate 27.5 g of water at 100°C (molar heat vaporization of liquid water = 4.07 x 10⁴ j/mol
62.1 kj
Consider the following balanced chemical equation: 3Ge(s) + 4HNO₃(l) → 3GeO₂(s) + 4NO(g) + 2H₂O(l) If 5.01 moles of Ge are completely reacted with HNO₃ to give 4.36 moles of NO₃, what is the percent yield of NO?
65%
How many joules are in 15.74 calories?
65.86 joules
What mass of sodium nitrate dissolved in 455 g of a solution that is 15.0% by mass NaNO₃?
68.3 g
If the pH of a coffee sample is 5.15, what is the H₃O+ concentration in the coffee?
7.1 x 10-⁶M
Consider the following balanced chemical equation: Zn(s) + 2O2(g) + 2S(s) -> ZnSO4(s) If 5.78 g of Zn are allowed to react with 3.00 g of O2 and excess sulfur, how many grams of ZnSO4 will be produced? The molar masses of Zn, O2, and ZnSO4 are 65.41, 32.00, and 161.48 g/mol, respectively.
7.57 g
The correct answer for the product (6.45 x 10⁵)x(1.2 x 10⁴)is: (considering significant figure)
7.7 x 10⁹
Mas percent of carbon in CH4
74.9%
A 4.24 g sample of a compound contains 3.22g carbon. what is the percent carbon in the sample?
75.9%
The number of neutrons in an atom of 1-131 is:
78
How many moles of K2SO4 are contained in 39.0 mL of 0.226 M K2SO4 solution?
8.85 x 10^-3 moles
Convert 1.13 atm to torr
859 torr
Consider the following balanced chemical equation: CaC2(s) + 2H2O(l) -> Ca(OH)2(s)+ C2H2(g) if 2.0 g of CaC2 are completely reacted with water to give 2.0 g of Ca(OH)2 what is the yield of Ca(OH)2? The molar masses of CaC2 and Ca(OH)2 are 64.1 and 74.1 respectively.
87%
Number if CO2 molecules present in 1.50 moles of CO2
9.03 x 10^23 molecules
Solve for the volume of 2.5 gallons of juice in units of m^3 (1 gal= 3.785 L)
9.5 x 10^-3m^3
Which of the following statements regarding orbitals is correct?
A 2P orbital is lower in energy than a 3P orbital
Pauli exclusion principle
A maximum of two electrons can occupy each orbital, and they must have opposite spins
Charles law states that the volume of a gas held at constant pressure is directly proportional to the absolute temperature. Which of the following is a consequence of Charle's law?
A sealed balloon will rise if the air in it is heated
Line spectrum
A set of distinct wavelengths of light that is unique for each element
A substance the ionizes to produce H+ ions when dissolved in water is called a _______?
Acid
In which of the following choices is the oxidation number incorrect? F₂(g); oxidation number = 0 K+ (aq); oxidation number 1+ Ag(s); oxidation number = 1+ Cl-(aq); oxidation number = 1- Cr³+(aq); oxidation number = 3+
Ag(s); oxidation number = 1+
What is the correct formula for the compound formed between the aluminum ion and the hydroxide ion?
Al(OH)₃
The formula for aluminum oxide is:
Al2O3
Elements that have only one electron in the highest energy s sublevel in their ground state are called?
Alkali metals
Consider the reaction 2HgO(s) → 2 Hg(l) + O₂(g). Which of the following statements is correct? Mercury is reduced Oxygen is Oxidized Oxide is the reducing agent Mercury(II) ion is the oxidizing agent All of these statements are correct
All of these statements are correct
Formula for aluminum oxide is:
Al₂O₃
What is the correct formula for the compound formed between the aluminum ion and the sulfide ion?
Al₂S₃
What metals react with a solution of HCI to produce H2 gas?
Any metal that appears above hydrogen in the activity series will react with acid to produce H2 - Chromium - Tin - Magnesium
Using periodic trends, arrange the following atoms in order of increasing electronegativity: F,O,S,As
As<S<O<F
A _____ is the smallest unit of an element that has the chemical properties of that element. Two or more of these units can be bound together in a discreet arrangement to form a _____.
Atom, Molecule
Balance the skeletal equation: Ba(NO₃)₂(aq) + K₂SO₄(aq) -> BaSO₄(s) + KNO₃ (aq)
Ba(NO₃)₂(aq) + K₂SO₄(aq) -> BaSO₄(s) + 2KNO₃ (aq)
The formula for Barium carbonate is:
BaCO3
A substance that reacts with an acid to form water is called a ______
Base
Which of these molecules or ions has a violation of the octet rule (other than H)?
BeF₂
When bromine becomes a monatomic ion, what is the formula?
Br-
In which compound does bromine have an oxidation number of 3+?
Br₂O₃
Molecular compounds contain which of the atoms?
C H N Cl
What ions, atoms, or molecules are present after CH₃CH₂OH(l) mixes with water?
CH₃CH₂OH(aq) and H₂O (l)
When acetate ion, CH₃CO₂-, reacts with water, what are the products?
CH₃CO₂H(aq) and OH-(aq)
Which of the following should be most soluble in ethanol, CH₃CH₂OH? I₂ C₆H₆ CCl₄ CO₂ CH₃NH₂
CH₃NH₂
Which of the following should be most soluble in ethanol, CH₃CH₂OH? CO₂ I₂ C₆H₆ CCl₄ CH₃NH₂
CH₃NH₂
Select the two BrØnsted-Lowry bases in the following equation: CH₃NH₂(aq) + H₂O(l) ⇌CH₃NH₃+ (aq) + OH- (aq)
CH₃NH₂ and OH-
Select the two BrØnsted-Lowry bases in the following equation: CH₃NH₂(aq)+ H₂O ⇌ CH₃NH₃+(aq) + OH-(aq)
CH₃NH₂ and OH-
Which of the following equations describes what happens when CH₃OH dissolves in water? CH₃OH(l)→CH₃OH(aq) 2CH₃OH(l)→ 2C(aq) + 4H₂(aq) + O₂(aq) CH₃OH(l)→C(aq) + 4H(aq) + O(aq) CH₃OH(l)→ C²-(aq) + 4H(aq) + O²-(aq) CH₃OH(l) +H₂O(l) → CH₅O₂H(l)
CH₃OH(l)→CH₃OH(aq)
What is the correct formula for the compound formed between copper (II) ion and the phosphide ion?
CU₃P₂
Calcium ion :
Ca2+
Which of the following is classified as an ionic compound? CaCO₃ CH₃OH all of these CF₄ NO₂
CaCO₃
Which of the following reactions is not an oxidation-reduction reaction? C(s) + CO₂(g)→ CO₂(g) CaCO₃(s) + 2HCl(aq) →CaCl₂(aq) + CO₂(g) + H₂O(l) CO(g) + Cl₂(g)→COCl₂(g) 2H₂O₂(l) →2H₂O(l) + O₂(g) 2HI(g) → H₂(g) +I₂(g)
CaCO₃(s) + 2HCl(aq) →CaCl₂(aq) + CO₂(g) + H₂O(l)
Products of combustion reaction Ca(s) + O2 (g)
CaO (s)
Metals that do not form cations of more than one charge
Cd Al Zn Sr Li - Metals in groups IA, IIA, IIIA, as well as certain transition metals such as Zn, Cd, and Ag, only form cations of one charge
The compound CIO3 s a dark brown solid powder that is not stable above 25°C. Name this molecular compound.
Chloride trioxide
Which element has the abbreviated ground state configuration: [Ne] 3s²3p⁵
Cl
Which species is a spectator ion in the following equation: 2Fe(s) +6HCI(aq) -> 2FeCl3(aq) + 3H2(g)
Cl-
Spectator ions in the following reaction BaCl2 (aq) -> Na2CO3 (aq) -> BaCO3 (s) +2 NaCl (aq)
Cl- (aq) Na+ (aq)
What is the chemical formula for the compound carbon tetraiodide?
Cl4
In which substance does chlorine have an oxidation number of 4+?
ClO₂
Which of the following has the strongest london dispersion forces? CF₄ CCI₄ CBr₄ CH₄ Cl₄
Cl₄
Products for following combustion reaction: C2H5)H(l) + O2 (g)
Co2 (g) H2O (g)
Co(OH)2
Cobalt (II) hydroxide
A + B -> AB
Combination - smaller components coming together to create a larger compound is a combination (synthesis) reaction
What are the oxidation numbers of the atoms in the atom Cr₂O₇²- ion?
Cr=6+, O=2-
Which of the following formulas for a compound containing Cr³+ ion is incorrect?
CrNO₃
Using periodic trends, arrange the following atoms in order of increasing electronegativity: S, Sr, P, Cs
Cs< Sr<P<S
Describe the process of CsF dissolving in water?
CsF(s) ->Cs+(aq) + F- (aq)
Which compound below is a base? C2H6 CsOH Fe(OH)2 LiOH
CsOH Fe(OH)2 LiOH
Ionic equation for: NaOH (aq) + Cu(NO3)2 (aq) -> 2NaOH3 (aq) + Cu(OH)2 (s)
Cu2+ (aq) + 2OH-(aq) -> Cu(OH)2(s)
Which of the following formulas for a compound containing the Cu²+ ion is incorrect?
CuN
Which of the following formulas for a compound containing CU²+ ion is incorrect? - CuP - CuSO4 - CuCO 3 - CuP - CuO
CuP
Which of the following is the correct formula for the compound with the name copper(II) sulfate?
CuSO₄
Identify any intermediates or catalysts in the following two-step reaction: Cu²+ + H₂ →CuH+ + H+ + H₂C = CH₂→Cu²+ + H₃C-CH₃
Cu²+ is a catalyst, CuH+ and H+ are intermediates
The formula for Copper (II) sulfide is:
Cu₂S
Which of the following contains a double bond? CH₄ C₂H₄ H₂ C₂H₂ C₂H₆
C₂H₄
Balance the following skeletal equation: C₂H₅OH(l) + O₂(g) -> CO₂ (g) + H₂O
C₂H₅OH(l) + 3O₂(g) -> 2CO₂ (g) + 3H₂O (g)
AB -> A + B
Decomposition - larger compound breaking up into smaller components
Name of compound N2O5
Dinitrogen pentoxide
Hund's Rule
Electrons are distributed into orbital of identical energy in such a way as to give the maximum number of unpaired electrons
Aufbau principle
Electrons fill orbitals starting with the lowest-energy orbitals
Which of the following elements is the most electronegative? F H P S Cl
F
Arrange the following bonds in order of increasing polarity: F-F, F-C,F-O, F-N
F-F<F-O<F-N<F-C
True or false: the empirical formula and the molecular formula of a compound are always the same
False
True or false: molecular compounds contain a combination of oppositely charged cations and atoms in a specific ration to produce a compound with a given whole-number charge.
False - ionic compounds do contain cations and anions in ratio of these components that gives an overall neutral (zero) charge
True or false: Only ionic compounds are solid at room temperature
False - molecular solids can also be solid at room temperature
Examine the following reactions: 5FeCl₂(aq) + KMnO₄ (aq) + 8HCl(aq) → 5FeCl₃(aq) + MnCl₂(aq) + KCl(aq) +4H₂O(l) Which element has undergone oxidation?
Fe
If you wish to make a sandwich which consists of two slices of bread, one ham slice, and three pickle pieces, how many sandwiches could you make if you have 12 slices of bread, five slices of ham, and 20 pickle slices, and what would be left over?
Five sandwiches could be made, 2 slices of bread and five pickle slices would be left over
Element name with the descriptive name of the group it belongs to from the periodic table:
Fluorine -> Halogen Magnesium -> Alkaline earth metal Lithium -> Alkali metal Argon -> Noble gas
Which of the following substances is most likely to be a gas at room temperature? Sr Mn CBr₄ C₆H₁₄ F₂
F₂
Main group elements
Groups 1,2, and 13-18
An acid is a substance that when dissolved in water produces which of the following?
H+
Products in the following chemical reaction: CH4(g) + 2O2(g) -> CO2(g) + O (g)
H20 CO2
Products of reactions between aqueous sodium hydroxide NaOH and sulfuric acid H2SO4
H2O (l) Na2SO4 (aq)
Products formed when two following solutions are mixed: HNO3(aq) + Na2CO3 (aq)
H2O (l) NaNO3 (aq) CO2 (g)
Products of combustion reactions of hydrocarbons (compounds that contain only carbon and hydrogen)
H2O(g) CO2(g)
Balance the following skeletal equation by counting and balancing polyatomic ions: H2SO4(aq) + KOH (aq) -> K2SO4 (aq) + H2O (I)
H2SO4(aq) + 2KOH (aq) -> K2SO4(aq) + H2O (I)
Which of the following contains a triple bond?
HCN
Which of the following contains a triple bond? O₃ NH₃ HCN C₂H₆ NO₃-
HCN
Which of the following is the strongest acid? NH⁴+, Ka= 5.6 x 10-¹⁰ HCO₂H, Ka= 1.8 x 10-⁴ CH₃CO₂H, Ka= 1.8 x 10-⁵ HCN, Ka= 6.2 x 10-¹⁰ HOCl, Ka= 4.0 x 10-⁸
HCO₂H, Ka= 1.8 x 10-⁴
Which of the following equations represents behavior of HCO₃- as an acid? HCO₃- (aq) +OH- (aq) ⇌ CO₃²-(aq) + H₂O(l) HCO₃- (aq) + H₂O(l) ⇌ H₂CO₃ (aq) + OH- (aq) HCO₃- (aq) + H₃O (aq) ⇌ H₂CO₃(aq) + H₂O (l) HCO₃- (aq) + HF (aq) ⇌ H₂CO₃(aq) + F- HCO₃-(aq) + HCN(aq) ⇌H₂CO₃(aq) + CN- (aq)
HCO₃- (aq) +OH- (aq) ⇌ CO₃²-(aq) + H₂O(l)
Which of the following equations describes what happens when HCl (g) dissolves in water?
HCl(g) -> H+ (aq) + Cl- (aq)
WHich of the following substances can participate in hydrogen bonding? CH₄ SiH₄ HF all of these choices are correct CH₃COCH₃
HF
Select the two brØnsted-lowry acids in the following equation: NH₃(aq) + HF(aq) ⇌ NH₄+ (aq) + F-(aq)
HF and NH₄+
Which of the following ionizes to the greatest extent? HCN, Ka= 6.2 x 10-¹⁰ HOCl, Ka= 4.0 x 10-⁸ CH₃CO₂, Ka=1.8 x 10-⁵ HF,Ka=6.3x 10-⁴ HCO₂H, Ka=1.8 x 10-⁴
HF,Ka=6.3x 10-⁴
Which of the following is the strongest acid? NH₄+, Ka = 5.6 x 10-¹⁰ CH₃CO₂H, Ka= 1.8 x 10-⁵ HCN, Ka= 6.2 x 10 -¹⁰ HNO₂, Ka = 5.6 x 10-⁴ HCO₂H, Ka= 1.8 x 10-⁴
HNO₂, Ka = 5.6 x 10-⁴
List the acid, base, conjugate acid, and conjugate base, in that order for the following reaction: HOCl(aq) +H₂O(l) ⇌ OCl-(aq) +H₃O+(aq)
HOCl, H₂O, H₃O, OCl-
Elements that have five electrons in the highest energy P sublevel in their ground state are called?
Halogens
Rank the following substances in order of increasing boiling point: F₂, Ne, He, Cl₂
He< Ne< F₂< Cl₂
Rank the following elements in order from increasing atomic size: Sr, He, Si, F
He<F<Si<Sr
_____ is the amount of energy that is transferred between two objects because of a difference in their temperatures.
Heat
The densities of ionic compounds are (higher/lower) _____ than the densities of molecular compounds
Higher
Acid with the formula HF
Hydrofluoric acid
IO-
Hypoiodite - Part of the family of oxoanions
Rank the following substances in order of increasing intermolecular forces: Ne,NH₃, H₂, O₂
H₂<Ne<O₂<NH₃
Select the pair that consists of an acid and it conjugate base in that order. NH₃/NH₄+ HPO₄²-/H₃PO₄ CO₃²-/CO₂²- CO₃²-/HCO₃- H₂CO₃/HCO₃-
H₂CO₃/HCO₃-
Which of the following has the highest boiling point H₂Se H₂Te H₂O H₂ H₂S
H₂O
Which of the following molecules is polar? CO₂ H₂S SO₃ CCl₄ BeF₂
H₂S
Select the pair that consists of an acid and its conjugate base in that order.
H₂SO₃/HSO₃-
Select the element that has a halogen in Period 5
I-
Which of the following formula/name combinations is incorrect?
ICl₇ iodine hexachloride
When acetylene, C₂H₂, a fuel used in welding, is burned in air, two molecules of acetylene combine with five oxygen molecules to form CO₂ molecules and two H₂O molecules. Select the statement below that is incorrect in regard to this reaction.
If 8 acetylene molecules react, 12 CO₂ molecules should form.
Net ionic equation
Includes only substances involved in the reaction
Which of the following changes will increase the average kinetic energy of the reactants? none of these choices increasing the surface area of the reactants adding a catalyst increasing the concentration of the reactants Increasing the temperature
Increasing the temperature
IO3-
Iodate - Part of the family of oxoanions
IO2-
Iodite - Part of the family of oxoanions
FeCO3
Ionic compound with a polyatomic ion
CuBr
Ionic compound with monatomic ions
MgBr2 is an _______ solid. Therefore be a relatively _____ solid.
Ionic, Hard
The compound FeI2 is a ____ compound. FeI2 will have a _____ melting point
Ionic, High
Spectator Ion
Ions that do not participate in the reaction, but are present in solution
Fe2(CO3)3
Iron (III) carbonate
Which element has three completely filled sublevels, one electron in it other s sublevel, and no d electrons in its ground state configuration?
K
Select the pair that has the largest atom or ion listed first: O, O²- O²-, Cl- N, N³- K+,Ca²+ Al³+, Al
K+,Ca²+
Which equilibrium constant represents a reaction that is product favored? not enough information Keq= 5.2 Keq= 8.4 x 10-⁵ Keq= 6.3 x 10-⁵ Keq=0.025
Keq= 6.3 x 10-⁵
Which of the following will not change when an acid is added to water? pOH pH Kw hydroxide ion concentration hydronium ion concentration
Kw
Based on the common charges, which formula for an ionic compound is incorrect? - Na₃N - K₂Cl - Li₂S - Mg(OH)₂ -CaO
K₂Cl
Monoatomic cations
Li+ - lithium ion, 1+ charge Ca2+ - Calcium ion, 2+ charge
Predict the molecular shape and give the approximate bond angle in the CO₂ molecule
Linear, 180°
The forces that hold CO₂ together in a solid state are
London Dispersion forces only
Which choice correctly lists the intermolecular forces present in CH₄
London forces only
Match the equation to the process involved for the ionization energy it represents (M=metal)
M(g) -> M+(g) + e- ==== first ionization energy M (g) -> M2+ (g) + e- ===== second ionization energy M (g) -> M3+ (g) + e- ===== third ionization energy
Hg2SO4
Mercury(I) sulfate
Compounds soluble in water
Mg(NO3)2 LiBr
Compound which could decompose to form MgO in a decomposition reaction
MgCO3
Product of a combination reaction between MgO and CO2
MgCO3
Which of the following formula/name pairs is incorrect?
MgCl₂ - Magnesium Dichloride
Based on the common charges, which formula for an ionic compound is incorrect? - KBr - Ba(NO₃)₂ - Al₂O₃ - MgCl₃
MgCl₃
The formula of the ionic compound that would be formed when magnesium and fluorine react is? MgF FMg Mg₂F F₂Mg MgF₂
MgF₂
Which element has the abbreviated ground state configuration: [Ar] s²3d⁵
Mn
Which element has the abbreviated ground-state electron configuration: [Ar] 4s² 3d⁵
Mn
PF5
Molecular compound
Ammonia (NH3) is a _____ compound. Ammonia (NH3) will have a _______ melting point.
Molecular, low
Dry ice (solid CO2) is a _____ compound. It is relatively _____ solid.
Molecular, soft - CO2 contains two nonmetals and therefore is a molecular compound
In which of the following bonds does nitrogen have a partial negative charge (δ-1)
N-C
In which of the following bonds does nitrogen have a partial negative charge(δ-)?
N-C
Formula of ionic compound formed between ammonium and fluoride ions
NH4F
All of the following are weak bases except: NH₃(aq) KF(aq) NH₄Cl(aq) CH₃NH₂(aq) Na₂CO₃(aq)
NH₄Cl(aq)
Which of the following components is likely to have covalent bonds?
NO2
Which of the following compounds is likely to have a covalent bond
NO2
Which of the following compounds is likely to have covalent bonds? BaCl₂ NO₂ LiBr Cr₂O₃ CsF
NO₂
Which of the following compounds is most likely to occur as a gas at room temperature?
NO₂
The correct symbol for the ion formed by sodium is:
Na+
Empirical formula for a compound composed if 21.5% Na, 33.3% CI, and 45.1% O by mass
NaCIO3
Products formed when aqueous solution of sodium phosphate Na3PO4 and magnesium chloride MgCl2 are mixed
NaCl (aq) Mg3(PO4)2 (s)
Which of the following is an amphoteric substance? CH₃OH NaCl NaHCO₃ KBr LiOH
NaHCO₃
NO2-
Nitrate ion - oxoanion
Which of the following combinations of formula and name is incorrect? Cyanide ion= CN- Perchlorate ion = ClO₄- Chloride ion = Cl- Nitride ion = NO₂- Chlorite ion= CIO₂-
Nitride ion = NO₂-
Elements that have six electrons in the highest-energy p sublevel in their ground state are called _________.
Noble Gases
A bulb connected to a battery through a solution of ethanol (CH3CH2OH) does not light up; ethanol is a ________ electrolyte. A bulb connected through a solution of calcium chloride (CaCL2) lights up brightly; calcium chloride is a ______ electrolyte.
Non, Strong
The correct formula for dinitrogen pentoxide is:
N₂O₅
Which of the following formula/name combination is incorrect?
N₂SO₅ - Dinitrogen Tetroxide
Consider the following balanced chemical equation 4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O (l) if 0.76 moles of NH₃ are reacted with 0.80 moles of O₂ what is the limiting reactant?
O₂
Consider the following balanced chemical equation: SiH₄(g) + 2O₂ →SiO₂(s) + 2H₂O(g) If 7 molecules of SiH₄ are allowed to react with 13 molecules of O₂ what is the limiting reactant?
O₂
Empirical formula for a compound containing 0.428 moles of P and 1.07 moles of O
P2O5
Which of the following molecules is polar? - PCI₃ - BF₃ - CS₂ - CH₄ - BeCl₂
PCI₃
Empirical formula for a compound that is 24.59% P and 75.41% F by mass
PF5
The formula for a phosphate ion is:
PO₄³-
The formula for phosphorus ion is:
PO₄³-
Rank the following elements in order from least to most number of moles of an atom in 10.0 g sample: Br,Fe,Pb,Hg
Pb<Hg<Br<Fe
What is the correct formula for the compound lead(IV) oxide?
PbO₂
BrO4-
Perbromate ion - oxoanion
IO4-
Periodate - Part of the family of oxoanions
K+ Cation
Potassium ion
The correct formula for tetraphosphorus hexasulfide is:
P₄S₆
Ionic equation
Represent substances as they actually exist in solution
Empirical formula of a compound that is composed of 0.24 moles of S and 0.48 moles of Cl
SCI2
Gaseous product formed from in the chemical reaction: 2HNO3(aq) + Na2SO3(aq) -> 2NaNO3 (aq) + H2O(I)
SO2(g)
Consider the reaction H₂O(l) + 3SO₃²- (aq) + 2MnO₄-(aq) →3SO₄²-(s) + 2MnO₂(s) + 2OH-(aq) Which species is the reducing agent?
SO₃²-
A + BC -> B + AC
Single- displacement - frequently involves the activity series, where the more active metals will displace/replace the less active metals in solution
The compound MgCl2 will be a (solid/liquid/gas) ________ at room temperature because it is an (ionic/molecular/ ________ compound.
Solid, Ionic
Which combination of formula and name is incorrect: Sr+ = strontium ion p3- = phosphide ion Li+ = lithium ion Br- = bromide ion S2- = sulfide ion
Sr+ = strontium ion
Rank the following in order of increasing ionization energy: Sr, He, Si, F
Sr<Si
What is the name of the compound with the formula Sr(OH)2
Strontium hydroxide
SO3^2-
Sulfite ion - oxoanion
Which ion is expected to be the largest? K+ Cl- all of these have the same size Ca²+ S²-
S²-
Which ion is expected to be the largest? S²- Ca²+ Cl- K+ all of these have same size
S²-
Describe physical properties:
Taste, Volume, and Melting point
Predict the molecular shape and give the approximate bond angles in the SiH₄ molecule
Tetrahedral 109.5°
Predict the molecular shape and give the approximate bond angles in the SiH₄ molecule.
Tetrahedral, 109.5°
Two balloons are at the same temperature and pressure, and contain equal volumes of gas, but one is floating, and the other is not. The reason for this behavior is that:
The balloon that is floating is more dense than the one that is not floating, so it holds up the balloon better
Ground state
The lowest energy state of an atom
Absolute Zero
The lowest possible temperature in the universe
Theoretical yield
The maximum amount of product that may be formed from a chemical reaction
Balanced equation
The number of atoms of a given element must be the same on both the product and reactant side of the equation
The mass of an atom represents
The number of protons and neutrons in that atom
Stoichiometry
The process of determining the amounts of substances in a chemical reaction
What occurs when a molecular solid dissolves in water?
The solid breaks into molecules which interact with water
Boiling Point
The temperature at which the liquid form of a substance changes to the gaseous form of a substance
Melting Point
The temperature at which the solid form of a substance changed to the liquid form
Which of the following statements is correct for a reaction in which Keq<<1?
There are more reactants than products at equillibrium.
Predict the molecular shape and give the approximate bond angles in the CO₃²- polyatomic ion.
Trigonal Planar, 120°
Predict the molecular shape and give the approximate bond angles in the SO₃ molecule
Trigonal Planar, 120°
Predict the molecular shape and give the approximate bond angles in the PCI₃ Molecule
Trigonal Pyramidal, 109.5°
Predict the molecular shape and give the approximate bond angles in the SO3²- polyatomic ion.
Trigonal Pyramidal, 109.5°
True or false: A molecular formula shows the actual number of each atom present in a given molecule
True
True or false: Knowing the charge on a polyatomic ion like carbonate is an important first step toward correctly writing a formula for an ionic compound
True
Which of the following statements regarding oxidation-reduction is correct? oxidation- reaction involves sharing electrons You can tell that a substance is oxidized if it loses electrons none of these statements are correct oxidation can occur without reduction. you can tell a substance is reduced if its oxidation number increases
You can tell that a substance is oxidized if it loses electrons
Consider the following reaction: Mg(s) + ZnSO₄(aq) → MgSO₄(aq) + Zn(s) Which of the following statements regarding the reaction is correct? Zinc gains two electrons magnesium is neither oxidized nor reduced the sulfate ion is reduced magnesium is the oxidizing agent zinc is the reducing agent
Zinc gains two electrons
Written name for ZnO is:
Zinc oxide
Electron configurations
Zn (Z=30): 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰ P (Z=15): 1s²2s²2p⁶3s²3p³ Ca (Z=20): 1s²2s²2p⁶3s²3p⁶4s² Ga (Z=31): 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p¹
What is the abbreviated ground state electron configuration for Sc
[Ar] 4s² 3d¹
Given an OH- concentration of 1.0 x 10-⁶ M, calculate the H₃O+ concentration, and then identify the solution as acidic, basic, or neutral.
[H₃O+]=1.0 x 10-⁸, basic
Given an OH- concentration of 1.00 x 10-⁴ M, calculate the H₃O+ concentration, and then identify the solution as acidic, basic, or neutral.
[H₃O] = 1.0 x 10-¹⁰, basic
Select the solution below that is the most acidic. [H₃O+] = 1.0 x 10-¹⁰ M [H₃O+] = 1.0 x 10-⁸ M [OH-] = 1.0 x 10-⁵ M [OH-] = 1.0 x 10-¹⁰ M
[OH-] = 1.0 x 10-¹⁰ M
Select the solution below that is the most basic. [OH-] = 1.0 x 10-⁵ M [OH-] = 1.0 x 10-⁴ M [OH-] = 1.0 x 10-⁹ M
[OH-] = 1.0 x 10-⁴ M
Endothermic reaction
a reaction that absorbs energy from the surroundings and is described as an "uphill" reaction
If the solubility of a solid substance is 18.2 g/100 g water, which of the following best describes what eventually forms after 10.0 grams of the substance is mixed with 50.0 grams of water?
a saturated solution with some undissolved solid
Continuous spectrum
a sequence of colors that contain all wavelength of light in the visible region
The substance Mg(OH)₂(aq) is
a strong base
The substance NH₃(aq) is
a weak base
White light
all the wavelengths of the visible spectrum at equal intensity
Consider the reaction: Ca(s) + 2H₂O(l)→Ca(OH)₂(aq) +H₂(g) Which of the following statements is correct? calcium is oxidized calcium is reduced oxygen is the reducing agent oxygen is oxidized hydrogen is oxidized
calcium is oxidized
CIO3-
chlorate ion
Classify the following reaction: 2C₈H₁₈(l) +25O₂(g) -> 16CO₂(g) + 18H₂O(g)
combustion
Which of the following statements regarding covalent bonding is incorrect? - most elements try to aquire an octet of electrons in their valence shell when bonding - hydrogen only requires two elements in its valence shell when bonding - in covalent bonding, electrons are shared between two atoms - it is possible for two atoms to share more than one pair of electrons - covalent bonds occur between a metal and a nonmetal
covalent bonds occur between a metal and a nonmetal
The law of conservation of energy states that energy may be converted from one form into another but it cannot be _______ nor ________.
created, destroyed
AB + CD -> AD + CB
double-displacement (metathesis) - positive ions will change places
What changes when an ion is formed from an atom?
electrons are lost or gained
An _______ reaction is a reaction in which the ______ contain less potential energy than the ______.
endothermic, products, reactants.
Units for molar mass
g/mole
Transition Elements
groups 3-12
The forces that hold CaF₂ together in the solid state are:
ionic bonds
what metal would act with an aqueous solution of copper (III) sulfate to produce copper metal
iron - iron is more active than copper
If a balloon filled with helium were heated with a blow dryer, the balloon would increase in volume. What would happen to the density of the helium in the balloon?
it would decrease
Inner-transition elements
lanthanides and actinides
Factors that influence reaction rates include all of the following except the: reaction temperature size of solid reactant particles concentration of reaction magnitude of the equilibrium constant
magnitude of the equilibrium constant
The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except____ - boiling point - viscosity - mass - vapor pressure - melting point
mass
Percent by mass concentration
mass solute/mass solution x 100%
The ____ ratio and the mole ratio are related to the coefficients in the chemical balanced equation.
molecule
Equation for calculating molarity (M) of a solution
moles of solute/L of solution
Mass of a substance given the number of moles
moles x molar mass mol of a substance x g/mol = g of a substance
Principle energy level with the orbitals found on that level
n=1 : s only n=2 : s and p only n=3 : s, p, and d only n=4 : s, p, d, and f only
A solid substance has a very low melting point, is soft and does not conduct heat or electricity. This substance is probably a(n) ______ solid.
nonpolar molecule
Equal volume of methane (CH₄) and hydrogen (H₂) gases under the same conditions of temperature and pressure have equal
number of molecules
Calculate the pH of a solution that has [H₃O+] = 1.0 x 10-⁷ M
pH= 7.00
Calculate the pH of a solution that has [OH-] = 1.0 x 10-⁶ M.
pH=8.00
Calculate the pH of a solution that has [OH-] = 5.9 x 10-⁵ M
pH=9.77
calculate the pOH of a solution that has [H3O+] = 5.2 x 10-⁷ M
pOH =7.72
A catalyst speeds up a chemical reaction by:
providing an alternate reaction pathway
Meanings of letter in equation: q= m x C x △T
q - heat m - mass C - specific heat △ T - temperature change
Molecular equation
represents all substances as if they exist as molecules (or formula units) in solution
Sublevel matched with description
s- a single-orbital that is the shape of a sphere p - three orbitals that are each in the shape of a dumbbell d - five orbitals in which four of them have four lobes and one of them has two lobes f - seven orbitals found only on the fourth principal energy level and above
Which of the following statements is incorrect? - the phase change from solid to gas is exothermic - since acetone (nail polish remover) evaporates more readily than water, one would assume that acetone has weaker intermolecular forces - a liquid which has a high boiling point has a higher vapor pressure at a given temperature than a liquid with a low boiling point. - liquids boil at higher temperatures in the mountains due to the higher altitude - evaporation is an exothermic process, since heat is given off when a substance vaporizes
since acetone (nail polish remover) evaporates more readily than water, one would assume that acetone has weaker intermolecular forces
NaBrO3
sodium bromate
NaBrO2
sodium bromite
NaBrO4
sodium perbromate
A ______ is a homogeneous mixture that is composed of a _______in a _______.
solution, solute, solvent
Which of the following compound names is not correct?
strontium dinitrate
The law of conservation states that the mass of the reactants must equal _____
the mass of the products
Which of the following statements regarding the nucleus of an atom is incorrect? - the nucleus contains the electrons and the protons - the nucleus contains the neutrons - the nucleus contains the neutrons and protons and most of the mass of the atom - the nucleus contains the most of the mass of an atom - the nucleus contains the central core of an atom
the nucleus contains the electrons and the protons
In any neutral atom:
the number of electrons is equal to the number of protons
The element Mg has three common isotopes: ²⁴Mg, ²⁵Mg, and ²⁶Mg. The differences between these three isotopes is:
the number of neutrons
The mass number of an atom represents
the number of protons and neutrons in that atom
If the value of q for a system is +3.5 kJ what change is occuring (if any)?
the system is gaining heat
The _____ yield is defined as the _____ amount of product that can be obtained from a chemical reaction.
theoretical, maximum
Which of the following is not a property of gases? - when gas particles collide, attractive forces keep them attached to one another - gases can be compressed in a container - gases consist of particles that are relatively far apart - gas particles collide with one another - when gases are stored under pressure, their densities increase
when gas particles collide, attractive forces keep them attached to one another
