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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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. 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
s orbital
atomic theory
Diprotic Base
Formal Charge
2. 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
Le chateliers Principle
molecular weight
Formula weight
Colligative properties
3. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
Planck's Constant
polymer
Nucleus
4. Chalcogens - - Oxide O
Group 6A
mole
quantum numbers
atomic theory
5. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
Hydrogen bonding
Solution equilibrium
London forces
6. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Noble gases
Halogens
Ion product
Vapor pressure
7. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Dipole
electrolysis
Le chateliers Principle
Diffusion
8. 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
Percent yield
Molality
Theoretical yield
9. 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
Pauli exclusion principle
Ionic Bond
Network covalent
Nucleus
10. 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.
physical reaction
Redox Half Reaction
Solute
Intermolecular forces
11. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Pauli exclusion principle
Common ion effect
empirical formula
12. The energy required to break a chemical bond and form neutral isolated atoms
quanta
Hydrogen bonding
atomic radius
bond energy
13. 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
azimuthal quantum number
Alkaline earths
compound
Planck's Constant
14. Rare earth element group (elements 58-71)
Raoult's Law
energy state
Ion
lathanide series
15. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
bond length
Free radical
quantum
Phase diagram
16. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Group 2A
STP
electromagnetic energy of photons emmited from electrons at ground state
sigma bond
17. A solution in which water is the solvent
Molarity
Octet Rule
Aqueous Solution
Effusion
18. PH of a molecule at which it contains no net electric charge - isoelectric point.
Disproportionation
atomic emission spectrum
VSEPR
pI
19. 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
Arrhenius Definition
Free radical
Emperical Formula
polymer
20. 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.
Lewis acid base reaction
STP
amorphous solid
crystalline solid
21. 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
quantum numbers
Reaction order
Atomic absorption Spectra
Hydrogen bonding
22. A subdivision of an energy level in an atom. They are divided into orbitals.
sigma bond
molecule
subshell
Henderson Hasselbalch Equation
23. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Acid dissociation constant
periodic trends
Activation energy
Group 6A
24. 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
pH
Effusion
Group 1A
Nucleus
25. The process of decomposing a chemical compound by the passage of an electric current.
Buffer
sigma bond
Group 6A
electrolysis
26. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Avagadros number
Water dissociation Constant
physical reaction
sigma bond
27. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
lathanide series
Ion
d orbital
representative elements
28. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
redox reaction
Aqueous Solution
atomic emission spectrum
Neutron
29. Substance in which a solute is dissolved to form a solution
Solvent
quantum numbers
chemical reaction
Electronegativity
30. Having characteristics of both an acid and a base and capable of reacting as either
Ion
Spin quantum number
Acid dissociation constant
Amphoteric
31. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Proton
Hydrogen bonding
Henry's Law
redox reaction
32. Common definition of acids as proton (H+) donors and bases as proton acceptors
Raoult's Law
Diprotic Base
Net ionic equation
Bronsted - Lowry definition
33. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Acid dissociation constant
Electronegativity
Group 6A
34. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
pi bonds
Bronsted - Lowry definition
atomic emission spectrum
Atomic absorption Spectra
35. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
theoretical yield
lewis base
Pauli exclusion principle
Solubility Product Constant
36. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Lyman series
s orbital
Network covalent
physical reaction
37. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
d orbital
bond energy
Formula weight
Raoult's Law
38. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Chemical Kinetics
Octet Rule
Rate law
bond length
39. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Bronsted - Lowry definition
Avagadros number
Theoretical yield
electrolysis
40. The Percent by mass of each element in a compound.
Raoult's Law
Equilibrium
Principle quantum number
Percent composition
41. 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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42. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.
Octet Rule
Lewis acid base reaction
atomic radius
amorphous solid
43. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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44. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Lewis acid base reaction
Half equivalence point
mole
Dipole Dipole interaction
45. The maximum amount of product that can be produced from a given amount of reactant
Mass number
Octet Rule
theoretical yield
Electronegativity
46. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
Equlibrium constant
Diprotic Base
Proton
lathanide series
47. Gram equivalent weight of solute per liter of solution - often denoted by N.
Nucleus
Ionization energy
Raoult's Law
Normality
48. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
STP
angular momentum in the bohr model
The bohr model
indicator
49. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Equivalence point
Bronsted - Lowry definition
Rate law
Aqueous Solution
50. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
Effective nuclear charge
Resonance structure
Activation energy
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