Hesi A2/ Chemistry Review
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Created by:
carmcbe on February 18, 2011
Subjects:
Description:
Review of chemistry for the hesi A2 nursing school entrance exam.
Classes:
HESI standardized test, Uintah Chemistry, HESI A2
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66 terms
Terms | Definitions |
|---|---|
 Homogeneous Mixture | Mixture with uniform density throughout and no distinguishable coponents. |
| Heterogeneous Mixture | Mixture in which the components are readily distinguished. |
| Physical Change | A change in which the checmical composition of a substance remains the same. |
| Chemical Change | A change in which the chemical bonds are broken and reformed to create a new and different substance. |
| Element | The simplest of substances and is represented by a specific letter or combinations of letters. |
| Compounds | Combinations of eleements in whole number ratios. |
| Law of Conservation of Mass | Mass cannot be created or destroyed during a chemical reaction. |
| Chemical Reaction | The breaking of bonds and the reforming of new bonds to create new chemical compounds with different chemical forumulas and different chemical properties. |
| Five main types of chemical reactions. | syntehesis, decomposition, combusion, single replacement, double replacement |
| Syntehsis Reaction | Two elements combine to form a product. |
| Decomposition Reaction | The breaking of a compound into component parts. |
| Combustion Reaction | The reaction of a compound or element with oxygen. In the combusiton of a hydrocarbon carbon dioxide and water are produced. |
| Replacement Reactions | Reaction involoving ionic compounds. The reactivity of the ionic compounds determines whether the reaction will take place or not. Can be single replacement or double replacement reaction. |
| Single Replacement Reaction | Reaction between a more active metal reacting with an ionic compound containing a less active metal to produce a new compound ex. copper wire reacting with aqueous silver nitrate. |
| Double Replacement Reaction | Reaction involving two ionic compounds where the positive ion from one compound combines with the negative ion of the other compound. The result it two new ionic compounds that have switches partners. |
| Atomic Number | The number of protons in a given element. |
| Atomic Weight/ Atomic mass number | An average of the masses of each of the iostopes of an element as they occur in mature. (Represents the number of protons and the number of neutrons in an element because electrons essentially have no mass). |
| Calculating the number of neutrons in a given isotope of an element. | Subtract the atomic number from the mass number. |
| Charge of Elements in Group IA | +1 |
| Charge of Elements in Group IIA | +2 |
| Charge of Elements in Group IIIA | +3 |
| How do you calculate density? | d = m/v |
| Specific Gravity | Density of an object realtive to water. No units. |
| Kinetic Energy | Energy of motion. |
| Potential Energy | Stored energy. |
| Heat | Form of energy, measured in calories. |
| calorie | The amount of heat necessary to raise the temperature of 1g of water by 1 degree celsius. |
| Mixture | Combination of two or more pure substances. |
| Isotope | Atoms with the same number of protons but different numbers of neutrons. |
| Noble Gases | Elements in group 8A of the periodic table. Have no charge and are gases under normal conditions. (Helium, Neon, Argon, Krypton, Xenon, Radon) |
| Electron Configuration | Shell Electrons (max) 1 2 2 8 3 18 4 32 |
| Halogens | Elements of group 7A. Have a charge of -1. Fluorine, Chlorine, Bromine, Iodine. Form compounds with sodium in the form NaX. |
| Alkali Metals | Elements of group 1A. Have a charge of +1. Lithium, Sodium, Potassium, Rubidium, Cesium. React with water to form hydrogen gas and a metal hydroxide (MOH) + H2. Also from compounds with the halogens in the form MX. Ex. NaCl. |
| Anion | An ion with a negative charge. |
| Cation | An ion with a positive charge. |
| Ionic bond | A chemical bond resulting from the attraction between a positive ion and a negative ion. |
| Covalent Bond | A chemical bond resulting from the sharing of electrons between two atoms. |
| Polar covlaent bond | A covalent bond between two atoms where electrons are not shared equally between the two atoms. |
| Dipole | Created when atoms are joined by a polar covalent bond. The positive end of a dipole in one compound will be attracted to the negative dipole in another compound creating weak attraction between the two compounds. |
| Strongest type of chemical bond. | Covalent bond |
| Weakest typ of chemical bond. | Ionic bond |
| Strongest of intermolecular forces. | Hydrogen bond |
| Weakest of intermolecular forces. | Dispersion forces. |
| Hydrogen bond. | Attraction for a hydrogen atom by a highly electronegative element. Generally involve fluorine, chlorine, oxygen, and nitrogen. |
| Dispersion Forces | Temporary dipole created when moving electrons within an element or compound concentrate themselves on one side of an atom. Usually found in nonpolar covalent compounds. |
| Van der Walls forces | Another name for dispersion forces, dipole interactions. |
| Charge of elements in group VA. | -3 |
| Charge of elements in group VI A | -2 |
| Charge of elements in group VII A | -1 |
| How many known elements are there? | 109 |
| What is a mole. | An amount of an element equal to its atomic weight in grams. Also described by the amount of a substance that contains 6.02 x 10 23rd particles of that substance. |
| What is alpha radiation? | The emission of helium ions that consist of 2 protons and 2 neutrons (thus having a +2 charge). Alpha particles can be stopped by a piece of paper. |
| What is beta radiation? | The product of the decomposition of a neutron and is composed of high energy high-speed electrons. They are negatively charged and have basically no mass. Beta particles can be stopped by aluminum foil. |
| What is gamma radiation? | High-energy electromagnetic radition that lacks charge and mass. Gamma radiation can be stopped by several feet of concrete or several inches of lead. |
| Radioactivity | The emission of particle sfrom an unstable nucleus. Exists in three forms alpha, beta, and gama radiation. |
| Molar mass | The mass of one mole of a compound. |
| Sublimation | When a substance changes from a solid to a gas without first becoming a liquid. |
| Ideal gas law | PV=nRT (n is equal to the number of moles of the substance and R is the gas constant 0.082) |
| Molarity | The number of moles of solute in 1 liter of solution. |
| Redox reactions | Reactions that involve the transfer of electrons from one element to another. |
| Oxidation | The loss of electrons in an redox reaction. |
| Reduction | The gain of electrons in a redox reaction. |
| Rules for determining oxidation state. | 1. Elemental atoms have an oxidation number of zero. 2. The oxidation number of any simple ion is the charge of the ion. 3. The oxidation number for oxygen in compound is always -2. 4. The oxidation number for hydrogen in compound is +1. 5. The sum of the oxidation numbers equals the charge on the molecule or polyatomic ions. |
| Acids | - act as hydrogen-ion donors - produce H3O+ in aqueous solutions - tast sour or tart - most of their formulas begin with H - relase H2 gas when reacting with active metals - conduct electrical current - pH is less than 7 |
| Bases | - produce OH- in solution - taste bitter - feel slippery -conduct electricity - formulas often contain OH- - pH is greater than 7 |
| Neutralization | Process which occurs when an acid and a base react tot produce a salt and water. The result is a pH near 7. |
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