SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Bronsted - Lowry definition
Proton
quantum
Ion dipole interactions
2. An elementary particle with 0 charge and mass about equal to a proton
Triple point
Neutron
Group 4A
Percent yield
3. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation
Free radical
Equlibrium constant
Molecular orbital
Spin quantum number
4. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water
lewis base
Arrhenius Definition
Spin quantum number
indicator
5. A substance that - when dissolved in water - results in a solution that can conduct electricity
mole
Electrolyte
atomic emission spectrum
Le chateliers Principle
6. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Equlibrium constant
Titration
Neutralization reaction
Activation energy
7. Small discrete increments of energy.
Charles and Gay Lussac's Law
Combination Reaction
Strong acid
quanta
8. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
decomposition reaction
Nonpolar covalent bond
Resonance structure
Covalent Bond
9. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Proton
Solubility Product Constant
Combination Reaction
indicator
10. Redox reaction - in which the same species is both oxidized and reduced.
Group 2A
Disproportionation
Period
Pauli exclusion principle
11. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
Le chateliers Principle
Diffusion
Colligative properties
Group 7A
12. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Mass number
atomic radius
periodic trends
Theoretical yield
13. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
und's rule
Balmer series
Lewis definition
14. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molecular orbital
und's rule
Activation energy
Avagadros number
15. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Group 7A
quanta
lewis base
Le chateliers Principle
16. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Colligative properties
redox reaction
chemical reaction
17. 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
d orbital
Group 7A
Resonance structure
Net ionic equation
18. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
Equlibrium constant
Dipole
Nonpolar covalent bond
19. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Avagadros number
Theoretical yield
Effective nuclear charge
Ionic Bond
20. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
quantum
Pauli exclusion principle
Formal Charge
Solubility Product Constant
21. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Ion product
Group 5A
STP
Buffer
22. Temperature is constant; effusion and temperature are proportional to the square root of their masses
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
23. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
molecule
quantum
heisenberg uncertainty principle
24. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Chemical Kinetics
Network covalent
Halogens
effective nuclear charge
25. Slightly less reactive than alkali metals - comprise group II
gram equivalent weight
und's rule
Azeotrope
Alkaline earths
26. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Le chateliers Principle
mole
Electronegativity
Lewis acid base reaction
27. The process by which one or more substances change to produce one or more different substances
und's rule
Solute
chemical reaction
Aqueous Solution
28. Tells you how much solute is present compared to the amount of solvent
Concentration
Free radical
Dipole
law of constant composition
29. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Diffusion
Rate law
Emperical Formula
Avagadros number
30. 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.
indicator
Atomic absorption Spectra
redox reaction
Disproportionation
31. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
redox reaction
single displacement reaction
Pauli exclusion principle
azimuthal quantum number
32. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Solute
sigma bond
atomic radius
Percent composition
33. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
34. A base that can accept two moles of H+ per mole of itself (ex: SO4
Henderson Hasselbalch Equation
Ionization energy
Diprotic Base
single displacement reaction
35. The average distance between the nuclei of two bonded atoms
bond energy
Diffusion
bond length
crystalline solid
36. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
transition elements
Molality
Noble gases
s orbital
37. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Buffer
Avagadros number
Formal Charge
subshell
38. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
lathanide series
representative elements
actinide series
39. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Bronsted - Lowry definition
angular momentum in the bohr model
Raoult's Law
theoretical yield
40. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Ionization energy
Graham's Law
actinide series
Theoretical yield
41. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
Covalent Bond
bond energy
Magnetic quantum number
Dispersion Forces
42. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Effusion
Common ion effect
Decomposition reaction
und's rule
43. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
heisenberg uncertainty principle
actinide series
Solubility Product Constant
Electronegativity
44. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Ionization energy
Diprotic Base
Principle quantum number
electron affinity
45. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Activation energy
Dipole Dipole interaction
Octet Rule
Net ionic equation
46. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
actinide series
decomposition reaction
Net ionic equation
gram equivalent weight
47. Sum of the protons and neutrons in an element often denoted by the letter A
Ion dipole interactions
The bohr model
Mass number
Group 7A
48. An atom or group of atoms that has a positive or negative charge
Group 1A
s orbital
Ion
Nonpolar covalent bond
49. The maximum amount of product that can be produced from a given amount of reactant
Concentration
Molality
theoretical yield
redox reaction
50. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Colligative properties
Electronegativity
Emperical Formula
atomic emission spectrum
Sorry!:) No result found.
Can you answer 50 questions in 15 minutes?
Let me suggest you:
Browse all subjects
Browse all tests
Most popular tests
Major Subjects
Tests & Exams
AP
CLEP
DSST
GRE
SAT
GMAT
Certifications
CISSP go to https://www.isc2.org/
PMP
ITIL
RHCE
MCTS
More...
IT Skills
Android Programming
Data Modeling
Objective C Programming
Basic Python Programming
Adobe Illustrator
More...
Business Skills
Advertising Techniques
Business Accounting Basics
Business Strategy
Human Resource Management
Marketing Basics
More...
Soft Skills
Body Language
People Skills
Public Speaking
Persuasion
Job Hunting And Resumes
More...
Vocabulary
GRE Vocab
SAT Vocab
TOEFL Essential Vocab
Basic English Words For All
Global Words You Should Know
Business English
More...
Languages
AP German Vocab
AP Latin Vocab
SAT Subject Test: French
Italian Survival
Norwegian Survival
More...
Engineering
Audio Engineering
Computer Science Engineering
Aerospace Engineering
Chemical Engineering
Structural Engineering
More...
Health Sciences
Basic Nursing Skills
Health Science Language Fundamentals
Veterinary Technology Medical Language
Cardiology
Clinical Surgery
More...
English
Grammar Fundamentals
Literary And Rhetorical Vocab
Elements Of Style Vocab
Introduction To English Major
Complete Advanced Sentences
Literature
Homonyms
More...
Math
Algebra Formulas
Basic Arithmetic: Measurements
Metric Conversions
Geometric Properties
Important Math Facts
Number Sense Vocab
Business Math
More...
Other Major Subjects
Science
Economics
History
Law
Performing-arts
Cooking
Logic & Reasoning
Trivia
Browse all subjects
Browse all tests
Most popular tests