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. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
heisenberg uncertainty principle
Common ion effect
Dipole Dipole interaction
Triple point
2. An elementary particle with 0 charge and mass about equal to a proton
amorphous solid
Ground state
Neutron
Raoult's Law
3. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
Henderson Hasselbalch Equation
Hydrogen bonding
Balmer series
Charles and Gay Lussac's Law
4. Chalcogens - - Oxide O
representative elements
STP
Group 6A
Alkaline earths
5. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Lyman series
Atomic weight
Ground state
Activation energy
6. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Ion
redox reaction
Ion
Group 6A
7. A substance that - when dissolved in water - results in a solution that can conduct electricity
Conjugate acids and Bases
heisenberg uncertainty principle
redox reaction
Electrolyte
8. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
subshell
London forces
Aqueous Solution
azimuthal quantum number
9. 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
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
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.
Molecular orbital
energy state
Lyman series
pi bonds
11. The average distance between the nuclei of two bonded atoms
Electronegativity
indicator
Buffer
bond length
12. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Le chateliers Principle
Equlibrium constant
atomic radius
pI
13. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
VSEPR
electron affinity
Alkaline earths
14. 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
Dipole
Solution equilibrium
Electrolyte
Halogens
15. 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
d orbital
Rate law
Ionization energy
Chemical Kinetics
16. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy
Group 5A
Group 4A
ionic cmpound
s orbital
17. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Vapor pressure
Conjugate acids and Bases
Lyman series
Rate determining step
18. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
representative elements
pi bonds
Balmer series
Ionization energy
19. The slowest elementary step which is the limit for the rate of the other steps
Solution equilibrium
Rate determining step
effective nuclear charge
Neutron
20. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Balmer series
Vapor pressure
Resonance structure
Halogens
21. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
pi bonds
heisenberg uncertainty principle
Molality
Activation energy
22. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
hydrogen bonding
Buffer
Dipole Dipole interaction
Phase diagram
23. Gram equivalent weight of solute per liter of solution - often denoted by N.
Avagadros number
Azeotrope
Normality
Equivalence point
24. 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
Formula weight
Resonance structure
energy state
The bohr model
25. Sum of the protons and neutrons in an element often denoted by the letter A
London forces
Collision theory of chemical Kinetics
Mass number
Formula weight
26. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
STP
Conjugate acids and Bases
Hydrogen bonding
mole
27. A reaction where a compound does Not change its molecular structure.
redox reaction
Colligative properties
physical reaction
Charles and Gay Lussac's Law
28. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points
Azeotrope
Phase diagram
Raoult's Law
energy state
29. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
Ion
Ionization energy
Group 7A
30. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
electromagnetic energy of photons emmited from electrons at ground state
subshell
Charles and Gay Lussac's Law
Avagadros number
31. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
d orbital
lewis base
Ionic Bond
Proton
32. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
mole
Resonance structure
Strong acid
Equivalence point
33. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Atomic absorption Spectra
Effusion
electron configuration
quantum
34. An ionic compound that resists changes in its pH
Molarity
d orbital
Graham's Law
Buffer
35. Two or more atoms held together by covalent bonds
Lewis structure
molecule
Solution equilibrium
energy state
36. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Molarity
gram equivalent weight
electromagnetic energy of photons emmited from electrons at ground state
molecular weight
37. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Bronsted Lowry
indicator
Decomposition reaction
redox reaction
38. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Emperical Formula
solvation
Conjugate acids and Bases
Decomposition reaction
39. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
lewis base
Rate law
Rydberg constant
40. A solid made up of particles that are not arranged in a regular pattern.
The bohr model
Ionization energy
percent composition
amorphous solid
41. 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
Group 1A
Half equivalence point
Ion product
Colligative properties
42. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
Solubility Product Constant
transition elements
Ion product
43. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital
Ionic Bond
Spin quantum number
amorphous solid
single displacement reaction
44. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
Electrolyte
Rate determining step
electron affinity
Group 3A
45. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
azimuthal quantum number
Dipole
effective nuclear charge
Amphoteric
46. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Period
Buffer
Molar solubility
47. The process by which one or more substances change to produce one or more different substances
Equilibrium
Covalent Bond
chemical reaction
Colligative properties
48. The process of decomposing a chemical compound by the passage of an electric current.
ionic cmpound
Balmer series
Rydberg constant
electrolysis
49. 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
50. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Chemical Kinetics
atomic radius
Dipole
Formula weight