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Test your basic knowledge |
MCAT Chemistry
Start Test
Study First
Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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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. E=hc/?
electromagnetic energy of photons emmited from electrons at ground state
VSEPR
Solvent
Ion product
2. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Triple point
atomic emission spectrum
Principle quantum number
transition elements
3. The lowest allowable energy state of an atom
empirical formula
Ground state
Henderson Hasselbalch Equation
Bronsted Lowry
4. 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
Nucleus
atomic radius
Aqueous Solution
mole
5. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
heisenberg uncertainty principle
compound
Group 3A
lathanide series
6. An atom or group of atoms that has a positive or negative charge
atomic emission spectrum
Conjugate acids and Bases
Ion
representative elements
7. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
physical reaction
Chemical Kinetics
London forces
Henderson Hasselbalch Equation
8. 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.
single displacement reaction
Balmer series
Colligative properties
Lewis acid base reaction
9. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Reaction mechanism
Ionic Bond
atomic theory
Atomic weight
10. The percent by mass of each element in a compound
polymer
percent composition
Intermolecular forces
Planck's Constant
11. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
azimuthal quantum number
Neutron
Formula weight
12. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
Electrolyte
Activation energy
Lewis definition
13. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
quanta
electron configuration
effective nuclear charge
indicator
14. Simplest whole # ration of atoms in a compound
Decomposition reaction
Emperical Formula
Ion dipole interactions
representative elements
15. 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
Decomposition reaction
heisenberg uncertainty principle
Proton
representative elements
16. Two or more atoms held together by covalent bonds
molecular weight
Atomic absorption Spectra
molecule
electrolysis
17. Property of the elements that can be predicted from the arrangement of the periodic table
Ground state
Chemical Kinetics
periodic trends
Lewis structure
18. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
heisenberg uncertainty principle
Molar solubility
Raoult's Law
19. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Magnetic quantum number
transition elements
Planck's Constant
20. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Disproportionation
quantum
Bronsted - Lowry definition
redox reaction
21. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Dispersion Forces
mole
Lewis structure
Solution equilibrium
22. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Equivalence point
Period
Neutralization reaction
23. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
quantum numbers
amorphous solid
Raoult's Law
24. 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
Triple point
Ionic Bond
compound
Atomic absorption Spectra
25. The process of decomposing a chemical compound by the passage of an electric current.
Group 1A
Octet Rule
amorphous solid
electrolysis
26. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Raoult's Law
Disproportionation
Ion dipole interactions
atomic emission spectrum
27. 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
Colligative properties
atomic radius
Le chateliers Principle
Intermolecular forces
28. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
Atomic weight
hydrogen bonding
Phase diagram
29. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Lyman series
Group 3A
Redox Half Reaction
30. 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.
Solubility Product Constant
Avagadros number
compound
molecular weight
31. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Graham's Law
Lyman series
redox reaction
s orbital
32. A solution in which water is the solvent
amorphous solid
Formula weight
Aqueous Solution
Colligative properties
33. A reaction where a compound does Not change its molecular structure.
Ion product
physical reaction
Titration
Ion dipole interactions
34. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Collision theory of chemical Kinetics
atomic radius
Theoretical yield
Reaction order
35. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Proton
empirical formula
Group 6A
d orbital
36. The process by which one or more substances change to produce one or more different substances
Equilibrium
chemical reaction
Dipole
Common ion effect
37. 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.
VSEPR
percent composition
Triple point
Graham's Law
38. 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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39. Gram equivalent weight of solute per liter of solution - often denoted by N.
quantum numbers
Normality
Electronegativity
lathanide series
40. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Lewis definition
und's rule
Ion
atomic radius
41. A subdivision of an energy level in an atom. They are divided into orbitals.
Solvent
azimuthal quantum number
subshell
mole
42. 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
Group 4A
VSEPR
Azeotrope
bond length
43. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
d orbital
Mass number
atomic radius
Octet Rule
44. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Decomposition reaction
effective nuclear charge
Concentration
Halogens
45. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Mass number
Lewis acid base reaction
electron affinity
The bohr model
46. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin
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47. 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
Rydberg constant
Ionization energy
Balmer series
Redox Half Reaction
48. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
single displacement reaction
Group 4A
angular momentum in the bohr model
Avagadros number
49. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Reaction order
Molar solubility
Titration
Group 2A
50. (chemistry) p(otential of) H(ydrogen)
pH
Phase diagram
Proton
azimuthal quantum number
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