Atoms and Elements
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| Atom | The smallest identifiable unit of an element
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| Law of Conservation of Mass | In a chemical reaction, matter is neither created not destroyed
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| Law of Definite Proportions | All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements
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| Law of Multiple Proportions | When two elements(call them A and B) form two different compounds, the masses of element B that combine with 1g of the element A can be expressed as a ratio of small whole numbers
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| 1. Atomic Theory | 1. Each element is composed of tiny, indestructible particles called atoms..
2. All atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements..
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| 2. Atomic Theory | 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 that they are bound together with other atoms
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| Electron | A negatively charged, low mass particle present within all atoms
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| Mass of Electron | 9.10x10^-28g
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| Radioactivity | The emission of small energetic particles from the core of certain unstable atoms
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| 1. Nuclear Theory | 1. Most of the atoms's mass and all of its positive charge are contained in a small core called the nucleus..
2. Most of the volume of that atom is empty space, throughout which tiny, negatively charged electrons are dispersed..
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| 2. Nuclear Theory | 3. There are as many negatively charged electrons outside the nucleus as there are positively changed particles(named protons) within the nucleus, so the atom is electrically neutral
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| Neutrons | Neutral particles within the nucleus
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| Atomic Mass Unit(amu) | Defined as 1/12 the mass of a carbon atom containing six protons and six neutrons
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| How are Elements Defined | An Element is defined by the number of protons it contains
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| Atomic Number(Z) | The number of protons in an atom's nucleus
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| Chemical Symbol | A one or two letter abbreviation listed directly below its atomic number on the periodic table
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| Isotopes | Atoms with the same number of protons but different numbers of neutrons. "Same element, different mass"
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| Natural Abundance of Isotopes | The percentage of the amount of a type of element found in a sample of those atoms
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| Mass Number(A) | The sum of the number of neutrons and protons in an atom.
A = number of protons(p) + number of neutrons(n)
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| Ions | Atoms that gain or lose electrons. Charged atoms
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| Cation | Positively charged ions. e^-1's < # P's
Ex: Li+
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| Anion | Negatively charged ions. e^-1's > # P's
Ex: F-
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| Periodic Law | When the elements are arranged in order of increasing mass, certain sets of properties recur periodically
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| Metals | Metals lie on the lower left side and middle of the periodic table and share common properties: they are good conductors of heat and electricity, malleable, can be drawn into wires(ductility), shiny, tend to lose electrons when undergo chemical changes.
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| Nonmetals | Lie on the upper right side of periodic table. Share varied properties: some are solids at room temperature, other are liquid or gases, all poor conductors of heat and electricity, all tend to gain electrons when undergo chemical changes
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| Metalloids | Exhibit mixed properties: several classified as semiconductors because of their intermediate(and highly temperature - dependent) electrical conductivity
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| Main Group Elements | Properties tend to be largely predictable based on their position in the periodic table. Labeled with a number and letter A
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| Transition Elements | Properties tend to be less predictable based simply on their position in the periodic table. Labeled with number and letter B
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| Family(group) Elements | Each column within the main-group regions of the periodic table
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| Noble Gases | Elements under group 8A. These are mostly unreactive
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| Alkali Metals | Group 1A elements. All reactive metals
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| Alkaline Earth Metals | Group 2A elements. Also all fairly reactive, although not quite as reactive as the alkali metals.
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| Halogens | Group 7A elements. Very reactive nonmetals.
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| Ions and the Periodic Table | A main-group metal tends to lose electrons, forming a cation with the same number of electrons as the nearest noble gas..
A main-group nonmetal tends to gain electrons, forming and anion with the same number of electron as the nearest noble gas
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| Atomic Mass | The average mass for each element
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| Calculating Atomic Mass | Atomic Mass of Element = (fraction of isotope 1 x mass of isotope 1) + (fraction of isotope 2 x mass of isotope 2) + (fraction of isotope 3 x mass of isotope 3) + ......
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| Mass Spectrometry | A technique that separates particles according to their mass
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| Mole(mol) | A mole is the amount of material containing
6.02214 x 10^23 particles. Called the chemist's "dozen". This number is called Avagadro's Number
1 mol = 6.02214 x 10^23 particles. This number is often rounded to *6.022 x 10^23*.
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| Mole Specific Value | The value of the mole is equal to the number of atoms in exactly 12 grams of pure carbon-12(12gC = 1 mol C atoms = 6.022x10^23 C atoms)
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| Molar Mass | The mass of 1 mol of atoms of an element. An element's molar mass in grams per mole is numerically equal to the element's atomic mass in atomic mass units. 1 amu = 1g/mol
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| Subatomic Particles | Three kinds...
1. Proton..
2. Neutron..
3. Electron
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| Proton(a.k.a. Atomic Number) | The number of protons is unique to each element..
Mass(AMU) = 1.00727
Relative Charge = +1
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| Neutron | Mass(AMU) = 1.00866
Relative Charge = 0
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| Electron | Don't affect mass..
Mass(AMU) = 0.00055
Relative Charge = -1
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| Charge of Zinc Ion | +2
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| Charge of Silver Ion | +1
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Created by:
TimChemistry1
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