134 Questions
Which of these elements is chemically similar to magnesium?
Calcium
What is the vapor pressure above a beaker containing a solution of NaCl that is made up of 250ml of water and 12g of NaCl?
23.4 mmHg
A smart phone has dimensions of 4.9 inches (height), 2.3 inches (width) and 8.0 millimeters (depth). What is the volume of the smart phone in cubic centimeters? (1 in = 2.54 cm)
58 cm3
What is the term used for findings that are summarized based on a pattern or trend?
Law
Which of the following is a tentative explanation for a set of observations?
Hypothesis
Plants use up copious amounts of which alkali metal, preventing most of it from being washed out to sea?
Potassium
Which of the following isotopes is likely to be the most stable?
Sn-50
What is the reducing agent in the following equation? Mg(s) + 2 HCl(aq) --> MgCl2(aq) + H2(g)
Mg
What is Avogadro's number?
The number of atoms in 12g of Carbon-12
What is the ratio of reactants and products in the chemical equation? NaOH + H2SO4 ==> Na2SO4 + H2O
2:1:1:2
Most nonmetallic elements are found in which block of the periodic table of elements?
P
Which arrangement accurately describes the standard entropy values for Na at different phases?
Na (s) < Na (l) < Na (g)
What element has been oxidized and what element has been reduced in the redox reaction shown? 3CuS + 8HNO3 ==> 3CuSO4 + 8NO + 4H20
Sulfur has been oxidized; nitrogen has been reduced
When iron ions react with water, is the iron ion acting like an acid or a base?
The iron ion is acting like an acid
Is either of the two major steps in the Haber-Bosch process considered an oxidation-reduction reaction?
Both of these steps are oxidation-reduction reactions
If the concentration of sulfuric acid is increased in a galvanic cell, will Ecell increase or decrease?
Ecell will decrease
Calculate the value of the standard Gibbs Free Energy change for the reaction CH3OH(l) + CO(g) --> CH3COOH(l). Is acetic acid thermodynamically stable compared with liquid water at standard conditions?
ΔG°rxn = -86.0 kJ; At standard conditions, acetic acid is less thermodynamically stable than water because it has a more negative value of ΔG°
What type of semiconductor would be produced by adding indium to silicon, and which element could produce the opposite type of semiconductor?
Doping silicon with indium produces a 'p-type' semiconductor; Adding arsenic to silicon would produce a 'p-type' semiconductor
What are atoms that have the same number of protons but different numbers of neutrons called?
Isotopes
Who proposed an atomic theory in 1808?
John Dalton
Who discovered the magnitude of the electron charge?
R.Millikan
What did E. Rutherford discover?
Nucleus
How are metals and non-metals separated in the periodic table?
Staircase
What are the horizontal rows in the periodic table called?
Periods
What is the reactant that is used up first in a chemical reaction called?
Limiting reagent
What is the term used to describe the concentration of a solution?
Molarity
What is the chemical formula of a compound determined from its molecular mass called?
Molecular Formula
A phase diagram is a diagram depicting the phases of a substance at different temperatures and pressures.
True
Phase change is a physical change involving a substance changing from one state of matter to another, such as liquid to gas.
True
Surface tension is the tendency of liquids to maximize their surface area.
False
Sublimation is a phase change involving a substance changing from solid directly to gas.
True
The solubility of ionic compounds in water is mainly determined by which of the following forces?
Ion-dipole
Solids can be divided into two categories, crystalline and...
Amorphous
The two types of close-packing are called cubic close-packing and...
Hexagonal
Three types of atomic solids are nonbonded, metallic, and...
Network covalent
Effusion is the transfer of gas through a small orifice into an evacuated chamber.
True
Kinetic molecular theory is a basic atomic model that describes the behavior of...
Gases
Boyle's law is a gas law that associates the product of the pressure and volume with the number of moles, temperature, and a universal proportionality constant.
True
Standard temperature and pressure are conditions defined as 0ºC and 1 atm.
True
The solubility of ionic compounds in water is mainly determined by which of the following forces?
Ion-dipole
An alloy is an example of a ... solution.
Solid-solid
The Tyndall effect is the effect whereby a colloidal solution interacts with electricity.
False
Raoult's law applies to a solution comprised of a non-volatile solute and is the relationship between the vapor pressure of the solution and the vapor pressure of the pure solvent.
True
Boiling point elevation is a colligative property that involves the increase in the boiling point of a solvent by the addition of a solute.
True
Colligative properties are concerned with the type of particles and not their number.
False
When a solid is dissolved in water and forms a solution that conducts electricity, the solid is called a(n)...
Electrolyte
Two dissolved ions in hard water are Mg2+ and...
Ca2+
When a solid comes out of a solution, the solid is called a(n)...
Precipitate
Acid-base reactions are also called...
Neutralization
Who defined an acid as a proton donor and a base as a hydroxide donor?
Arrhenius
A reaction where electrons are transferred from one reactant to another is called a...
Redox or oxidation-reduction
What is the term for the phenomenon where two electrons in the same orbital must have opposite spins?
Pauli exclusion principle
How many electrons can p-orbitals hold at most?
Six
How many electrons can d orbitals hold at most?
Ten
What is the actual nuclear charge minus the charge from the core electrons called?
Effective nuclear charge
Unreactive gases that have a full valence shell of electrons are known as...
Noble gases
A reduction in atomic radii caused by the 4f electrons being close to the nucleus is called...
Lanthanide contraction
What are the two particles that compose the nucleus?
Neutrons and Protons
What is the charge of a proton?
positive
What is the charge of a neutron?
neutral
What is the charge of an electron?
negative
Are protons and electrons equal in charge?
equal
What is a derived unit?
A unit defined by a combination of SI units
Who proposed the Atomic Theory in 1803?
John Dalton
Who discovered the nucleus?
Ernest Rutherford
Who discovered the magnitude of the electron charge?
R.Millikan
Who proposed the "plum pudding" model of the atom?
JJ Thomson
What is Raoult's Law?
relationship between the vapor pressure of a solution and the vapor pressure of the pure solvent
Define Boiling Point Elevation.
the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent
Which two ions are dissolved in hard water?
Mg2+ and Ca2+
What is the definition of a Precipitate?
When a solid comes out of a solution
What are Acid-base reactions also called?
neutralization reactions
How did Arrhenius define acids and bases?
Defined acids as proton donors and bases as hydroxide donors
What is Redox or Oxidation-Reduction?
reaction where electrons are transferred from one reactant to another
Define Orbital.
plot of the wavefunction squared that gives the probability map of the electron's position
What is Wavelength?
the distance between the wave peaks and troughs
What is Amplitude?
the magnitude of a wave; in sound, the primary determinant of loudness
What is a Node?
Point in wavefunction where the electron cannot be found
What is an Emission Spectrum?
radiation that is emitted by atoms
What determines an atom's electron configuration?
specific orbitals that electrons occupy
Explain the Pauli Exclusion Principle.
Two electrons in the same orbital must have opposite spins
Define Valence Electrons.
Electrons on the outermost energy level of an atom
What is the element essential for plant growth?
potassium
What do Group 1A elements have in terms of charge?
1+
What do Group 2A elements have in terms of charge?
2+
What do Group 3A elements have in terms of charge?
3+
What do Group 4A elements have in terms of charge?
4-
What do Group 5A elements have in terms of charge?
3-
What do Group 6A elements have in terms of charge?
2-
What do Group 7A elements have in terms of charge?
1-
What is the formula for Zinc Iodide?
ZnI2
What is done to the formula if a cation and anion have different charge values?
Swap the charge numbers and put them as subscripts
What is the name of NF3?
Nitrogen Trifluoride
What is the name of N2O4?
Dinitrogen Tetroxide
What is the molecular formula for Carbon Disulfide?
CS2
What is the molecular formula for Dinitrogen Trioxide?
N2O3
What is the molecular formula for Sulfur Tetrafluoride?
SF4
What is the molecular formula for Tetraphosphorus Decasulfide?
P4S10
What is the empirical formula for C6H12O6?
CH2O
All elements fall into one of the following groups: ____, ____, ____
metal, nonmetal, metalloid
What does the mass number equal to?
number of protons + number of neutrons
What is the number below an element on the periodic table?
Atomic Weight
What is the number above an element on the periodic table?
Atomic Number
What are Alpha rays?
Positively charged particles that are deflected away from the positively charged plate
What are Beta rays?
Electrons that are deflected away from the negatively charged plate
What are Gamma rays?
high energy radiation that have no charge and are unaffected by external electric or magnetic fields
What are Strong Acids?
HCl, HBr, HI, HNO3, H2SO4, HClO4, HClO3, HSO4
What is the formula for the mass of an Electron?
charge/(charge/mass)
What is the charge of Element+?
Minus one electron
What is the charge of Element-?
plus one electron
What should be done if a cation and anion have different values in their charge for the formula?
Swap the charge numbers and put them as subscripts
What does 'Mono' represent?
1
What does 'Di' represent?
2
What does 'Tri' represent?
3
What does 'Tetra' represent?
4
What does 'Penta' represent?
5
What is the scientific name for NF3?
Nitrogen Trifluoride
What is the proper name for N2O4?
Dinitrogen Tetroxide
What is the molecular formula for Carbon Disulfide?
CS2
What is the molecular formula of Dinitrogen Trioxide?
N2O3
What is the molecular formula for Sulfur Tetrafluoride?
SF4
What is the molecular formula for Tetraphosphorus Decasulfide?
P4S10
What is the empirical formula for C6H12O6?
CH2O
Calculate the number of moles in 47.51 g of Al2O3.
0.4660 mol
Known to form complexes with platinum that inhibit the growth of cancerous cells, what is the systematic name for [CoCl3(H2O)]-?
Aquatrichlorocobaltate(II)
In K4[Fe(CN)6], how many 3d electrons does the iron atom have?
6
Write the formula for diamminedichloroethylenediaminecobalt(III) bromide.
[CoCl2(en)(NH3)2]Br
In the complex ion [Co(en)2Br2]+, what is the oxidation number of Co?
+3
In which type of isomerism is there restricted rotation around a bond?
Geometrical isomers
What name is given to a compound containing a -CONH2 group?
Amide
Bromination of benzene (C6H6) occurs by substitution rather than addition.
True
The density of a substance is an intensive property.
True
The rusting of a piece of iron under environmental conditions is a physical change.
False
77 K is colder than 4 K.
False
Study Notes
Here are the study notes:
Chemistry
- StraighterLine Chemistry Final Exam 2024-2025
Elements and Compounds
- Calcium is chemically similar to magnesium.
- Iron(III) ion has an electron configuration of [Ar]3d5.
- Phosphorus has a hybridization of sp3 in the PCl4+ cation.
Atomic Structure
- Effective nuclear charge is less than the actual nuclear charge due to shielding.
- Electron configuration of an element with ns2np1 outermost electrons is in group 3A.
Molecular Geometry
- Molecular geometry of ammonia (NH3) is trigonal pyramidal.
- AB5 molecules with one lone pair on the central atom have a square pyramidal molecular geometry.
Stoichiometry
- Mass of one copper atom is 1.055 × 10-22 g.
- Percent sulfur in iron(III) sulfate is 24%.
- Micrograms in 65.3 kg is 6.53 × 1010 μg.
Chemical Bonding
- CS2 is a covalent compound.
- Molecular geometry of a molecule with one lone pair on the central atom is trigonal pyramidal.
Periodic Table
- Electron configuration of gold is [Xe]4f145d106s1.
- Characteristics of isotopes were described.
- Atomic mass unit is a unit of mass equal to one-twelfth the mass of a carbon-12 atom.
Spectroscopy
- Emission spectra can be used to identify unknown atoms.
- Different types of spectra were described.
Acids and Bases
- A strong acid is H2SO4.
- Equilibrium constant for the autoionization of water at 25°C is 1.0 × 10-14.
- Amphiprotic species include Al2O3.
Gases
- Conditions of STP are 273.15 K and 760 torr.
- Van der Waals equation was described, including the constants a and b.
Intermolecular Forces
- Hydrogen bonding occurs in CH3CH2OH.
- Dispersion forces are stronger in krypton than in argon.
- Types of intermolecular forces were described.
Solubility and Solutions
- Henry's law states that the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution.
- An unsaturated solution is one that contains less solute than it has the capacity to dissolve.
- Solubility of a gas in a liquid is affected by pressure, temperature, and nature of the solute and solvent.Here are the study notes:
Selective Precipitation
- The principle of selective precipitation is used to identify the types of ions present in a solution.
- It is also known as qualitative analysis.
Acid-Base Indicators
- Methyl red is a common acid-base indicator.
- It has a Ka equal to 6.3 × 10-6.
- The un-ionized form of methyl red is red, and its anionic form is yellow.
- At a pH of 7.8, a methyl red solution would be yellow.
Titration
- When a strong acid is titrated with a weak base, the pH at the equivalence point is less than 7.0.
- A spontaneous endothermic reaction always causes the surroundings to get colder.
Nuclear Chemistry
- 123I is used to image the brain.
- Nuclear power plants do not pollute the air with SO2, soot, and fly-ash.
- Californium-249 is used to obtain dubnium-260.
- Sr-92 is used to obtain an isotope with atomic number 121 and mass number 299.
Coordination Compounds
- The name given to a compound containing a -CONH2 group is an amide.
- Bromination of benzene occurs by substitution rather than addition.
- The rusting of a piece of iron under environmental conditions is a chemical change.
- Lewis theorized the octet rule to describe chemical bonding where atoms lose, gain, or share electrons in order to achieve a noble gas configuration.
Physical Chemistry
- Matter is anything that has mass and occupies space.
- Atomic size decreases across a period due to an increase in the effective nuclear charge (Zeff).
- The radii of ions are not always smaller than the radii of the corresponding atoms of the same element.
General Chemistry
- The correct formula for the dibromobis(oxalato)cobaltate(III) ion is not [Co(C2O4)Br2]3+.
- The maximum oxidation state of an element in the first transition series never exceeds its group number.
- In complexes of transition metals, the maximum coordination number of the metal is not equal to its number of d electrons.
- A complex ion that undergoes a very slow exchange reaction is called an inert complex.
Isotopes and Radioactivity
- Sn-50 is the most stable isotope among F-21, Kr-77, Po-210, and Sn-50.
- Ernest Rutherford disproved J.J. Thomson's plum-pudding model of the atom by showing that positive matter is concentrated in the central core.
- Avogadro's number is the number of atoms in 12g of Carbon-12.
Let me know if you'd like me to reorganize or clarify any of these points!### Acid-Base Reactions
- Iron ions can act as acids or bases, depending on the definition used (Brønsted-Lowry, Lewis, or Arrhenius)
- In the reaction Fe3+(aq) + 3H2O(l) → Fe(OH)3(s) + 3H+(aq), the iron ion is acting as an acid, accepting a pair of electrons from the oxygen
The Haber-Bosch Process
- The Haber-Bosch process is used to produce ammonia (NH3) from nitrogen and hydrogen
- The process involves two steps:
- CH4(g) + H2O(g) → 2H2(g) + CO(g)
- 3H2(g) + N2(g) → 2NH3(g)
- Both steps are oxidation-reduction reactions
Galvanic Cells
- The galvanic cell involves two half-reactions:
- HSO4-(aq) + Pb(s) → H+(aq) + PbSO4(s) + 2e- (Eo = +0.35 V)
- PbO2(s) + 3H+(aq) + HSO4-(aq) + 2e- → PbSO4(s) + 2H2O(l) (Eo = +1.46 V)
- Increasing the concentration of sulfuric acid will increase the Ecell of the galvanic cell
Thermodynamics
- The standard Gibbs Free Energy change (ΔG°rxn) can be calculated for a reaction
- In the reaction CH3OH(l) + CO(g) → CH3COOH(l), ΔG°rxn = -86.0 kJ
- Acetic acid is less thermodynamically stable than water at standard conditions
Enzyme Activity
- Enzyme activity can be inhibited by the product of the reaction binding to the active site on the enzyme
- This inhibition can be biologically useful in preventing over-production of the product
Semiconductors
- Doping silicon with indium produces a p-type semiconductor
- The indium has fewer valence electrons than silicon, producing positively charged "holes" in the electron structure
Atomic Theory
- Isotopes are atoms of the same element that have different numbers of neutrons
- The nucleus of an atom is composed of protons and neutrons
- The charge of a proton is positive, while the charge of a neutron is neutral
Phase Changes
- Sublimation is a phase change involving a substance changing from solid directly to gas
- A phase diagram is a diagram depicting the phases of a substance at different temperatures and pressures
Solutions
- The solubility of ionic compounds in water is mainly determined by ion-dipole forces
- An alloy is an example of a solid-solid solution
- Molarity is a concentration term that uses the volume of a solution
This quiz is based on the final exam questions and answers of Straighterline Chemistry course, covering various topics in chemistry. It's a comprehensive assessment of chemistry knowledge, suitable for students looking to pass with an A+ grade.
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