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Test your basic knowledge |
MCAT Chemistry
Start Test
Study First
Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can
study here
.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.
This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.
1. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
Conjugate acids and Bases
electron configuration
Percent yield
Intermolecular forces
2. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
representative elements
Formula weight
Graham's Law
Solution equilibrium
3. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Covalent Bond
d orbital
Lewis structure
Phase diagram
4. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
crystalline solid
Neutron
Period
The bohr model
5. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
actinide series
VSEPR
Arrhenius Definition
atomic theory
6. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Atomic weight
Molarity
Net ionic equation
Conjugate acids and Bases
7. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.
pI
Resonance structure
Atomic absorption Spectra
subshell
8. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Atomic absorption Spectra
Ionic Bond
Magnetic quantum number
Triple point
9. A reaction where a compound does Not change its molecular structure.
Equlibrium constant
physical reaction
hydrogen bonding
electrolysis
10. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
gram equivalent weight
Lyman series
Bronsted Lowry
Charles and Gay Lussac's Law
11. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electrolyte
Molarity
Ionization energy
Group 4A
12. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
theoretical yield
molecule
Lewis structure
heisenberg uncertainty principle
13. Gram equivalent weight of solute per liter of solution - often denoted by N.
Avagadros number
crystalline solid
Ionic Bond
Normality
14. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
atomic radius
Effusion
Group 1A
Lyman series
15. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Neutron
Magnetic quantum number
VSEPR
16. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
Spin quantum number
Ion
Colligative properties
s orbital
17. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
Triple point
quantum
Group 1A
18. The maximum amount of product that can be produced from a given amount of reactant
Dipole
Phase diagram
Acid dissociation constant
theoretical yield
19. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
Decomposition reaction
atomic emission spectrum
Balmer series
Rate law
20. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities
The bohr model
Nucleus
Magnetic quantum number
Diffusion
21. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
angular momentum in the bohr model
Collision theory of chemical Kinetics
Spin quantum number
22. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Emperical Formula
Ion product
Formula weight
Free radical
23. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
azimuthal quantum number
atomic radius
single displacement reaction
24. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
Combination Reaction
Buffer
Theoretical yield
Magnetic quantum number
25. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Common ion effect
Proton
sigma bond
26. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
quantum numbers
Triple point
und's rule
27. Numbers that specify the properties of atomic orbitals and of their electrons
Solute
Halogens
quantum numbers
atomic emission spectrum
28. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
angular momentum in the bohr model
Ion
bond energy
Percent composition
29. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
Atomic absorption Spectra
electrolysis
Covalent Bond
30. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
Buffer
lathanide series
Effective nuclear charge
31. The process of decomposing a chemical compound by the passage of an electric current.
Solvent
electrolysis
Henry's Law
solvation
32. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Theoretical yield
Molality
Diffusion
33. A base that can accept two moles of H+ per mole of itself (ex: SO4
Combination Reaction
energy state
Formula weight
Diprotic Base
34. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
pH
Avagadros number
Solution equilibrium
Chemical Kinetics
35. (chemistry) p(otential of) H(ydrogen)
Group 4A
pH
Vapor pressure
Molecular orbital
36. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Normality
lewis base
Ion product
Vapor pressure
37. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
Titration
Period
s orbital
Strong acid
38. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Octet Rule
Equilibrium
Decomposition reaction
hydrogen bonding
39. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
electrolysis
Balmer series
Halogens
40. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture
bond length
Colligative properties
Solution equilibrium
Effusion
41. Simplest whole # ration of atoms in a compound
Effective nuclear charge
Activation energy
Ion
Emperical Formula
42. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
empirical formula
Avagadros number
Strong acid
Water dissociation Constant
43. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Period
Noble gases
Redox Half Reaction
quantum
44. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
single displacement reaction
hydrogen bonding
Solvent
45. The process by which one or more substances change to produce one or more different substances
chemical reaction
Strong acid
Azeotrope
Reaction mechanism
46. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
Molar solubility
Group 6A
Ion product
Formal Charge
47. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion
Net ionic equation
Molar solubility
Resonance structure
Raoult's Law
48. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
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49. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
decomposition reaction
Atomic absorption Spectra
Pauli exclusion principle
atomic theory
50. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
The bohr model
Concentration
Halogens
Collision theory of chemical Kinetics