Flashcards on Test on Chemistry Final
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| What are electrons? |
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| Negatively charged subatomic particles that exist on the outside of the nuclei of atoms |
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| What was Dalton's Atomic Theory? |
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| 1) All elements are composed of tiny invisible particles called atoms. 2) Atoms of the same element are identical. The atoms of any one element are different from those of any other element. |
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| Define protons. |
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| Positively charged subatomic particles located inside the nucleus of an atom. They have the same mass as neutrons. |
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| Define neutrons. |
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| Subatomic particles with no charge whatsoever, but with a mass nearly equal to that of a proton. They too are located inside the nucleus of an atom. |
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| Which scientist tested a theory of atomic structure using alpha particles and a sheet of gold foil? |
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| Ernest Rutherford in 1911. |
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| What is the atomic number? |
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| The number of protons in the nucleus of an atom of that element. |
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| What is the mass number? |
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| The total number of protons and electrons in an atom. |
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| What are isotopes? |
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| Atoms that have the same number of protons but different numbers of neutrons. |
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| How much is one amu? |
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| 1/12th the mass of a Carbon-12 atom. |
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| How much is one amu? |
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| 1/12th the mass of a Carbon-12 atom. |
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| Define atomic mass. |
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| The weighted average f the atoms in a naturally occurring sample of the element. |
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| What is the periodic table? |
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| The periodic table is an arragement |
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| What is a chemical formula? |
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| A formula which shows the kinds of numbers of atoms in the smallest representative unit of the substance. |
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| What is a molecular formula? |
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| A formula which shows the kinds and numbers of atoms present in a molecule of a compound. |
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| Define formula unit. |
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| The lowest whole-number ratio of ions in the compound. |
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| State the Law of Definite Proportions |
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| In samples of any chemical compound, the mases of the elements are always in the same proportions. |
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| State the Law of Multiple Proportions |
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| Whenever two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers. |
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| What are monatomic ions? |
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| Ions that consist of only one atom. The charges can be determined through the periodic table. |
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| Define polyatomic ions. |
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| Tightly bound groups of atoms that behave as a unit and carry a charge. |
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| H2PO4- |
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| Dihydrogen Phosphate |
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| C2H3O2- |
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| Acetate |
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| HSO3- |
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| Hydrogen Sulfite |
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| HSO4- |
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| Hydrogen Sulfate |
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| HCO3- |
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| Hydrogen Carbonate |
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| NO2- |
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| Nitrite |
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| NO3- |
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| Nitrate |
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| CN- |
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| Cyanide |
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| OH- |
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| Hydroxide |
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| MnO4- |
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| Permanganate |
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| ClO- |
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| Hypochlorite |
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| ClO2- |
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| Chlorite |
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| ClO3- |
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| Chlorate |
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| ClO4- |
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| Perchlorate |
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| HPO42- |
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| Hydrogen Phosphate |
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| C2O42- |
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| Oxalate |
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| SO32- |
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| Sulfite |
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| SO42- |
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| Sulfate |
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| CO32- |
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| Carbonate |
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| CrO42- |
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| Chromate |
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| Cr2O72- |
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| Dichromate |
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| SiO32- |
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| Silicate |
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| PO33- |
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| Phosphite |
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| PO43- |
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| Phosphate |
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| NH4+ |
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| Ammonium |
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| List the prefixes used to name Binary Molecular Compounds starting with "Mono" for 1. |
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| HCl |
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| Hydrochloric Acid |
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| H2SO4 |
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| Sulfuric Acid |
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| HNO3 |
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| Nitric Acid |
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| HC2H3O2 |
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| Acetic Acid |
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| H3PO4 |
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| Phosphoric Acid |
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H2CO3 |
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| Carbonic Acid |
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| Define a mole. |
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| A mole is a unit of meausrement like a dozen, which represents 6.02x1023 representative particles of a substance |
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| What is Avagadro's number? |
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| 6.02x1023 |
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| What is the Gram Atomic Mass (gam)? |
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| The atomic mass of an element expressed in grams. |
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| Gram formula mass (gfm) |
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| The mass of one mole of an ionic compound. |
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| Define Molar Mass |
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| The mass (in grams) of one mole of the substance |
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| What is the molar volume of a gas (at STP)? |
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| 22.4L |
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| Define Percent Composition. |
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The relative amounts of each element in a compound.
Or by the percent by mass of each element in a compound. |
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| What is the use of the Empirical Formula? |
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| It gives the lowest whole-number ratio of the atoms of the elements in a compound. |
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| How do you determine the molecular formula from the empirical formula? |
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| What are reactants? |
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| The substanes on the left hand side of a chemical equation. |
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| What are products? |
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| The substances on the right hand side of the chemical equation. |
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| What happens in a combination reaction? |
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| Two or more substances combine to become a single substance. The reactants are either two elements or two compounds. |
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| What happens in a decomposition reaction? |
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| A single compound is broken down into two or more products. They can be any combination of elements and compounds. |
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| What happens in a single replacement reaction? |
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| One element replaces a second element in a compound. (A.K.A. Single Displacement). Whether or not one element will replace another one is determined by the activity series of metals table. |
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| What happens in a double replacement reaction? |
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Double replacement reactions involve an exchange of positive ions between two reacting compounds.
One of the following rules must be true for this type of reaction to occur:
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| What happens in a combustion reaction? |
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An element or a compound reacts with oxygen, often producing energy as heat and light. These reactions commonly include hydrocarbons, compounds of hyrdrogen and carbon.
O2 will always be a reactant. |
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| Define Valence Electrons |
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| Electrons in the highest occupied energy level of an element's atoms |
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| State the octet rule. |
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| In forming compounds, atoms tend to achieve the electron configuration of a noble gas. An octet is a set of eight. |
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| What are electron dot structures? |
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| Electron dot structures are diagrams that illustrate valence electrons as dots. |
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| What are ionic bonds? |
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| The forces of attraction that bind cations and anions (oppositely charged ions) |
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| What is a single covalent bond? |
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| A bond in which two atoms share a pair of electrons. |
