Term
| The Law of the Conservation of Mass |
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Definition
| In a chemical reaction, matter is neither created nor destroyed. In other words, the sum of the masses of the reactants will always be equal to the sum of the masses of the products. |
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Term
| The Law of Definite Proportions |
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Definition
| A law formulated by Joseph Proust which states that all samples of a given compound have the same proportions of their constituent elements. |
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Term
| The Law of Multiple Proportions |
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Definition
| A law formulated by John Dalton after having noticed that whenever two elements are involved in a compound with one another, the amount of the second element paired with a fixed amount of the first element will, when put into ratios with one another, work out to be a ratio of small, whole numbers. This law stated that when two elements, A and B, form two compounds, the masses of element B that combine with 1g of element A can be expressed as a ratio of small whole numbers. |
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Term
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Definition
| A theory of atoms proposed by John Dalton in which there are the three following concepts: - Each element is composed of tiny, indivisible, indestructible particles called atoms. -All atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements. 3. Atoms combine in simple, whole number ratios to form compounds. 4. Atoms of one element cannot change into atoms of another element. In a chemical reaction, atoms only change the way they are bound together with other atoms. |
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Term
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Definition
Rutherford's Theory of the Atom that differed from JJ Thomson's Plum Pudding model of the atom, which had three main points:
-Most of the atom's mass and all of its positive charges are contained in a small core called the nucleus.
-Most of the volume of the atom is empty space, thoughout which tiny, negatively charged electrons are disperesed.
- There are as many negatively charged electrons outside the nucleus as there are positively charged particles (named protons) within the nucleus, so that the atom is electrically neutral. |
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Term
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Definition
| The number of protons of an element, expressed as Z in notations. |
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Term
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Definition
| The law formulated by Mendeleev that spurred him to create the first version of the periodic table, which states that when elements are arranged in order of increasing mass, certain sets of properties recur periodically. |
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Term
| Characteristics of Metals |
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Definition
-Luster
-Malleable
-Ductile
-Good conductor of heat and electricity
-All are solid at room temperature except Mercury
-Loses electrons in chemical reactions |
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Term
| Characteristics of Non-Metals |
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Definition
-Poor conductors
-Gains electrons in chemical reactions
-All three states of matter exist at room temperature |
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Term
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Definition
-Semi-conductors, meaning that its powers of conduction are dependent on temperature.
-The ability to change and control the conductivity makes them good materials to be used in electronics. |
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Term
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Definition
| Those columns in the periodic table that have predictable characterisitcs in their elements according to their placement on the periodic table. |
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Term
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Definition
| Those elements on the periodic table that belong to columns where their characterisitcs cannot be easily known from their position on the periodic table. |
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Term
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Definition
| 8A, inert gases with filled electron shells. |
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Term
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Definition
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Term
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Definition
| 2A, fairly reactive metals. |
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Term
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Definition
| The average mass of an element's isotopes |
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Term
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Definition
| A method that can measure the masses of atoms and their percent abundances. |
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Term
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Definition
| 6.022 x 10^23, the number used to define one mole, defined in terms of the number of atoms in 12 grams of Carbon-12. |
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Term
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Definition
| The mass of one mole of an element in grams per mole, |
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Term
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Definition
| The set of chemical properties associated with metals, resulting from how readily metals lose their electrons. |
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Term
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Definition
| The energy required to remove an electron, of which Helium has the most. |
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Term
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Definition
| The size of the atom, which is largely dependent on how much space the electrons take up or how far the valence electrons are from the nucleus. |
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Term
| Metallic Character Trends |
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Definition
| Metallic character decreases L to R because atoms want to work on filling their shells rather than losing a shell as they gain more electrons in the valence shell. Metallic character increases from T to B because the valence electrons that are growing to be farther apart from the positively charged nucleus as more electron shells are added have less attraction to hold them to the atom, and thus are more readily lost. |
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Term
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Definition
| Atomic size increases from top to bottom because more shells are added, known as "N." |
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Term
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Definition
| The charge a valence electron feels from the protons in the nucleus after "screening" the closer electrons -- meaning after feeling the repulsion of their negative charge. |
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Term
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Definition
| Z Effective does not change as you move up and down because the newly added shells are simply repelled by the inner electron shells, despite the newly added protons. Z effective increases as you move from left to right because the newly added electrons will not be perfectly shielded by inner shells and will increase the charge that valence electrons feel from the protons. |
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Term
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Definition
| Atomic Radius decreases from left to right because the stronger attraction between the electrons and the nucleus will make the atom smaller. |
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Term
| What is amu equivalent to? |
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Definition
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Term
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Definition
| Very reactive non-metals that are trying to get for electrons. |
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Term
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Definition
| The number of protons and neutrons in an atom. |
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Term
| Name match: Antoine Lavoisier |
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Definition
| Law of Conservation of Mass |
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Term
| Name match: Joseph Proust |
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Definition
| Law of Multiple Proportions |
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Term
| Name match: JJ Thomson proposed... |
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Definition
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Term
| Name match: John Dalton proposed... |
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Definition
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Term
| Name match: Rutherford proposed... |
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Definition
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Term
| Name match: JJ Thomson discovered... |
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Definition
| the electron with a cathode ray tube |
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Term
| Name match: Rutherford discovered... |
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Definition
| layout of atom by shooting particles into gold foil. |
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Term
| Name match: Millikan discovered... |
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Definition
| charge of electron through the oil drop experiment. |
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Term
Name the following components:
A
X
Z |
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Definition
A = mass number
Z = atomic number
X = chemical symbol |
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Term
| How can you figure out how many electrons ions of main group non-metals will have? |
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Definition
| They will have the same amount as the nearest noble gas. |
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Term
| How do you convert amu to grams? |
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Definition
6.022 x 1023 amu = 1 gram
so....
X amu / 6.022 x 1023 amu = grams |
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Term
| What is another word for column? |
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Definition
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