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. 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
Balmer series
Alkaline earths
Charles and Gay Lussac's Law
Arrhenius Definition
2. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Proton
ionic cmpound
Formal Charge
Ion dipole interactions
3. An atom or group of atoms that has a positive or negative charge
Raoult's Law
Ion
Halogens
pI
4. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Common ion effect
Atomic weight
Diffusion
Lewis definition
5. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
atomic radius
pi bonds
Group 4A
Aqueous Solution
6. 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
Electronegativity
pi bonds
Equilibrium
Nucleus
7. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Formal Charge
Group 3A
Acid dissociation constant
Group 1A
8. Named after their cation and anion
ionic cmpound
Bronsted Lowry
Half equivalence point
Strong acid
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
Vapor pressure
Ionic Bond
representative elements
electromagnetic energy of photons emmited from electrons at ground state
10. Simplest whole # ration of atoms in a compound
atomic theory
Emperical Formula
law of constant composition
compound
11. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Planck's Constant
Reaction mechanism
Common ion effect
Ion
12. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Resonance structure
decomposition reaction
Effusion
Covalent Bond
13. An ionic compound that resists changes in its pH
Triple point
chemical reaction
Buffer
Azeotrope
14. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
Percent composition
Avagadros number
Arrhenius Definition
Group 3A
15. 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
Effusion
Acid dissociation constant
Nonpolar covalent bond
indicator
16. 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.
Henderson Hasselbalch Equation
percent composition
crystalline solid
redox reaction
17. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
Pauli exclusion principle
Electronegativity
Redox Half Reaction
18. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Solubility Product Constant
subshell
atomic radius
Conjugate acids and Bases
19. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
Bronsted Lowry
hydrogen bonding
Molarity
20. 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
Charles and Gay Lussac's Law
law of constant composition
Hydrogen bonding
Equlibrium constant
21. 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.
Equivalence point
Buffer
Octet Rule
Nucleus
22. 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.
Net ionic equation
Solubility Product Constant
transition elements
representative elements
23. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
24. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Redox Half Reaction
angular momentum in the bohr model
heisenberg uncertainty principle
atomic emission spectrum
25. 5 valence electrons -3 ions - Nitride N
Ionic Bond
Group 5A
heisenberg uncertainty principle
indicator
26. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
single displacement reaction
azimuthal quantum number
Group 6A
Lewis structure
27. Gram equivalent weight of solute per liter of solution - often denoted by N.
Net ionic equation
pi bonds
electromagnetic energy of photons emmited from electrons at ground state
Normality
28. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
pI
Ion
redox reaction
Balmer series
29. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Charles and Gay Lussac's Law
hydrogen bonding
atomic emission spectrum
Nonpolar covalent bond
30. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Half equivalence point
polymer
Disproportionation
lewis base
31. A solution in which water is the solvent
Molality
Water dissociation Constant
actinide series
Aqueous Solution
32. 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.
Henderson Hasselbalch Equation
Net ionic equation
Percent yield
Lewis structure
33. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Effective nuclear charge
compound
Avagadros number
Molar solubility
34. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Triple point
Reaction order
Molecular orbital
Diffusion
35. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Dipole
Conjugate acids and Bases
Equilibrium
polymer
36. 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
subshell
single displacement reaction
Raoult's Law
Resonance structure
37. The energy required to break a chemical bond and form neutral isolated atoms
redox reaction
bond energy
Theoretical yield
subshell
38. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Equivalence point
Group 2A
lewis base
bond length
39. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Charles and Gay Lussac's Law
crystalline solid
Dipole Dipole interaction
Water dissociation Constant
40. In a solution - the substance that dissolves in the solvent
Conjugate acids and Bases
Solute
STP
energy state
41. Slightly less reactive than alkali metals - comprise group II
Formal Charge
Alkaline earths
Percent yield
The bohr model
42. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Disproportionation
Emperical Formula
Activation energy
Arrhenius Definition
43. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
44. A reaction in which atoms of one element take the place of atoms of another element in a compound
Equivalence point
Common ion effect
Group 5A
single displacement reaction
45. A base that can accept two moles of H+ per mole of itself (ex: SO4
Formula weight
Diprotic Base
Common ion effect
Period
46. A subdivision of an energy level in an atom. They are divided into orbitals.
Vapor pressure
transition elements
subshell
Neutralization reaction
47. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Reaction order
solvation
Bronsted Lowry
pH
48. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Electronegativity
electron configuration
Rate determining step
Buffer
49. 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
Lewis structure
Electronegativity
hydrogen bonding
Colligative properties
50. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
single displacement reaction
Molality
Lyman series
electromagnetic energy of photons emmited from electrons at ground state