Calculating the number of neutrons in a given isotope of an element.
Front
Subtract the atomic number from the mass number.
Back
Strongest type of chemical bond.
Front
Covalent bond
Back
Potential Energy
Front
Stored energy.
Back
Hydrogen bond.
Front
Attraction for a hydrogen atom by a highly electronegative element. Generally involve fluorine, chlorine, oxygen, and nitrogen.
Back
Charge of Elements in Group IIIA
Front
+3
Back
Anion
Front
An ion with a negative charge.
Back
Weakest typ of chemical bond.
Front
Ionic bond
Back
Charge of Elements in Group IIA
Front
+2
Back
Weakest of intermolecular forces.
Front
Dispersion forces.
Back
Van der Walls forces
Front
Another name for dispersion forces, dipole interactions.
Back
Isotope
Front
Atoms with the same number of protons but different numbers of neutrons.
Back
Combustion Reaction
Front
The reaction of a compound or element with oxygen. In the combusiton of a hydrocarbon carbon dioxide and water are produced.
Back
Noble Gases
Front
Elements in group 8A of the periodic table. Have no charge and are gases under normal conditions. (Helium, Neon, Argon, Krypton, Xenon, Radon)
Back
Covalent Bond
Front
A chemical bond resulting from the sharing of electrons between two atoms.
Back
Electron Configuration
Front
Shell Electrons (max)
1 2
2 8
3 18
4 32
Back
Homogeneous Mixture
Front
Mixture with uniform density throughout and no distinguishable coponents.
Back
Decomposition Reaction
Front
The breaking of a compound into component parts.
Back
How many known elements are there?
Front
109
Back
Element
Front
The simplest of substances and is represented by a specific letter or combinations of letters.
Back
Five main types of chemical reactions.
Front
syntehesis, decomposition, combusion, single replacement, double replacement
Back
Compounds
Front
Combinations of eleements in whole number ratios.
Back
Halogens
Front
Elements of group 7A. Have a charge of -1. Fluorine, Chlorine, Bromine, Iodine. Form compounds with sodium in the form NaX.
Back
Ionic bond
Front
A chemical bond resulting from the attraction between a positive ion and a negative ion.
Back
Charge of elements in group VI A
Front
-2
Back
Atomic Weight/ Atomic mass number
Front
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).
Back
Charge of Elements in Group IA
Front
+1
Back
How do you calculate density?
Front
d = m/v
Back
Law of Conservation of Mass
Front
Mass cannot be created or destroyed during a chemical reaction.
Back
Dipole
Front
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.
Back
Heat
Front
Form of energy, measured in calories.
Back
Replacement Reactions
Front
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.
Back
Single Replacement Reaction
Front
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.
Back
Chemical Change
Front
A change in which the chemical bonds are broken and reformed to create a new and different substance.
Back
Alkali Metals
Front
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.
Back
Polar covlaent bond
Front
A covalent bond between two atoms where electrons are not shared equally between the two atoms.
Back
Double Replacement Reaction
Front
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.
Back
Strongest of intermolecular forces.
Front
Hydrogen bond
Back
Charge of elements in group VA.
Front
-3
Back
Physical Change
Front
A change in which the checmical composition of a substance remains the same.
Back
Syntehsis Reaction
Front
Two elements combine to form a product.
Back
Dispersion Forces
Front
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.
Back
calorie
Front
The amount of heat necessary to raise the temperature of 1g of water by 1 degree celsius.
Back
Heterogeneous Mixture
Front
Mixture in which the components are readily distinguished.
Back
Mixture
Front
Combination of two or more pure substances.
Back
Specific Gravity
Front
Density of an object realtive to water. No units.
Back
Chemical Reaction
Front
The breaking of bonds and the reforming of new bonds to create new chemical compounds with different chemical forumulas and different chemical properties.
Back
Section 2
(16 cards)
Acids
Front
- 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
Back
Radioactivity
Front
The emission of particle sfrom an unstable nucleus. Exists in three forms alpha, beta, and gama radiation.
Back
Sublimation
Front
When a substance changes from a solid to a gas without first becoming a liquid.
Back
What is a mole.
Front
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.
Back
Reduction
Front
The gain of electrons in a redox reaction.
Back
Molarity
Front
The number of moles of solute in 1 liter of solution.
Back
Oxidation
Front
The loss of electrons in an redox reaction.
Back
Molar mass
Front
The mass of one mole of a compound.
Back
What is alpha radiation?
Front
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.
Back
Rules for determining oxidation state.
Front
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.
Back
Redox reactions
Front
Reactions that involve the transfer of electrons from one element to another.
Back
What is gamma radiation?
Front
High-energy electromagnetic radition that lacks charge and mass. Gamma radiation can be stopped by several feet of concrete or several inches of lead.
Back
Bases
Front
- produce OH- in solution
- taste bitter
- feel slippery
-conduct electricity
- formulas often contain OH-
- pH is greater than 7
Back
Neutralization
Front
Process which occurs when an acid and a base react tot produce a salt and water. The result is a pH near 7.
Back
What is beta radiation?
Front
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.
Back
Ideal gas law
Front
PV=nRT (n is equal to the number of moles of the substance and R is the gas constant 0.082)