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Chapter 2
Atoms and Elements
| Term | Definition |
|---|---|
| Atom | The smallest identifiable unit of an element |
| Law of Conservation of Mass | In a chemical reaction, matter is neither created not destroyed |
| 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 |
| 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 |
| 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.. |
| 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 |
| Electron | A negatively charged, low mass particle present within all atoms |
| Mass of Electron | 9.10x10^-28g |
| Radioactivity | The emission of small energetic particles from the core of certain unstable atoms |
| 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.. |
| 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 |
| Neutrons | Neutral particles within the nucleus |
| Atomic Mass Unit(amu) | Defined as 1/12 the mass of a carbon atom containing six protons and six neutrons |
| How are Elements Defined | An Element is defined by the number of protons it contains |
| Atomic Number(Z) | The number of protons in an atom's nucleus |
| Chemical Symbol | A one or two letter abbreviation listed directly below its atomic number on the periodic table |
| Isotopes | Atoms with the same number of protons but different numbers of neutrons. "Same element, different mass" |
| Natural Abundance of Isotopes | The percentage of the amount of a type of element found in a sample of those atoms |
| Mass Number(A) | The sum of the number of neutrons and protons in an atom. A = number of protons(p) + number of neutrons(n) |
| Ions | Atoms that gain or lose electrons. Charged atoms |
| Cation | Positively charged ions. e^-1's < # P's Ex: Li+ |
| Anion | Negatively charged ions. e^-1's > # P's Ex: F- |
| Periodic Law | When the elements are arranged in order of increasing mass, certain sets of properties recur periodically |
| 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. |
| 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 |
| Metalloids | Exhibit mixed properties: several classified as semiconductors because of their intermediate(and highly temperature - dependent) electrical conductivity |
| Main Group Elements | Properties tend to be largely predictable based on their position in the periodic table. Labeled with a number and letter A |
| Transition Elements | Properties tend to be less predictable based simply on their position in the periodic table. Labeled with number and letter B |
| Family(group) Elements | Each column within the main-group regions of the periodic table |
| Noble Gases | Elements under group 8A. These are mostly unreactive |
| Alkali Metals | Group 1A elements. All reactive metals |
| Alkaline Earth Metals | Group 2A elements. Also all fairly reactive, although not quite as reactive as the alkali metals. |
| Halogens | Group 7A elements. Very reactive nonmetals. |
| 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 |
| Atomic Mass | The average mass for each element |
| 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) + ...... |
| Mass Spectrometry | A technique that separates particles according to their mass |
| 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*. |
| 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) |
| 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 |
| Subatomic Particles | Three kinds... 1. Proton.. 2. Neutron.. 3. Electron |
| Proton(a.k.a. Atomic Number) | The number of protons is unique to each element.. Mass(AMU) = 1.00727 Relative Charge = +1 |
| Neutron | Mass(AMU) = 1.00866 Relative Charge = 0 |
| Electron | Don't affect mass.. Mass(AMU) = 0.00055 Relative Charge = -1 |
| Charge of Zinc Ion | +2 |
| Charge of Silver Ion | +1 |
Created by:
TimChemistry1
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