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Physics of the Earth CP Test: 11/20/09 Review for Unit 4 Test: Matter and Chemistry The Periodic Table- A table arrangement of the elements according to their atomic numbers so that elements with similar properties are in the same column. Rows – Horizontal, Left to Right, also known as a period Columns- Vertical, Up and Down, also known as groups or families Group Number- The group number is the number assigned to the vertical columns of the structured list of all known elements in the periodic table. Elements within the same group have the same number of electrons in their outer electron shells. Thus, all elements in the same group have similar chemical properties. Groups in the Periodic Table- The elements are arranged in the sequence of their increasing atomic numbers into the periodic table, which is arranged in rows and columns, so that elements with similar chemical properties are in the same vertical column. Families- A group or family is a vertical column in the periodic table. Groups are considered the most important method of classifying the elements. Non Metals- Any of a number of elements, such as oxygen or sulfur, that lack the physical and chemical properties of metals Alkali Metals- Any of a group of soft, white, low-density, lowmelting, highly reactive metallic elements, including lithium, sodium, potassium, rubidium, cesium, and francium. Alkaline Metals- Any of a group of metallic elements, especially calcium, strontium, magnesium, and barium, but generally including beryllium and radium. Transition Metals- Any of the metallic elements within Groups 3 to 12 in the Periodic Table that have an incomplete inner electron shell and that serve as transitional links between the most and the least electropositive in a series of elements. Metalloids- A nonmetallic element, such as arsenic, that has some of the chemical properties of a metal. A nonmetallic element, such as carbon, that can form an alloy with metals. Halogens- Any of a group of five chemically related nonmetallic elements including fluorine, chlorine, bromine, iodine, and astatine. Nobel Gases- Any of the elements in Group O of the periodic table, including helium, neon, argon, krypton, xenon, and radon. Other Metals- The 7 elements classified as "other metals" are located in groups 13, 14, and 15 of the Periodic Table. All of these elements are solid, have a relatively high density and are opaque. The "Other Metals" on the Periodic Table are: Aluminum, Gallium, Indium, Tin , Thallium, Lead, Bismuth Rare Earth Metals: are located in Group 3 of the Periodic Table and in the 6th and 7th periods. The Rare Earth Elements are of the Lanthanide and Actinide series. Most of the elements in the Actinide series are synthetic or man-made. Protons, Neutrons, Electrons- sub-atomic particles Protons- positively charged sun atomic particle Neutrons- no charge but contributes mass Electrons- lightest, a stable sub-atomic particle Charges, MassesCounting subatomic particles in atomsMass Number- add protons and neutrons Atomic Number- is the number of protons in an atom. The number of protons is unique for each element. No two elements have the same atomic number. Example: Carbon has six protons and an atomic number of 6. Oxygen has eight protons and an atomic number of 8. Chemical Symbol- is a one- or two-letter code used to represent an element. Each element has its own chemical symbol. Example: C always represents Carbon, Na always represents Sodium, Fe always represents Iron Valence Electrons- An electron in an outer shell of an atom that can participate in forming chemical bonds with other need 8 for stability. Example: Nobles Gases have all eight and are reluctant to bond Ions- gain or loss of an electron Isotopes- different neutrons, atoms of the same element Chemical Symbols- found on the periodic table, represented by letters or symbols Classifying Matter- matter is anything that has mass or volume Mixture- A composition of two or more substances that are not chemically combined with each other and are capable of being separated. Pure Substance- A chemically pure substance is a kind of matter that cannot be separated into other kinds of matter by any physical or chemical process. It has the same color, taste, texture and composition at a given temperature Element- A substance composed of atoms having an identical number of protons in each nucleus. Elements cannot be reduced to simpler substances by normal chemical means. Compound- A pure, homogeneous substance consisting of atoms or ions of two or more different elements in definite proportions that cannot be separated by physical means. A compound usually has properties unlike those of its constituent elements. Heterogeneous- Consisting of dissimilar elements or parts example: Homogeneous Mixtures- A composition of two or more substances that are not chemically combined with each other and are capable of being separated. Physical vs. Chemical Changes and Properties Physical Change- A physical change can be changed back to its original form. A physical change is any change not involving a change in the substance's chemical identity. Physical Property- Physical properties are those that can be observed without changing the identity of the substance. The general properties of matter such as color, density, hardness, are examples of physical properties. Example: water can be changed into ice and ice can be changed back to water, its original form. Or Tearing magnesiaum Chemical Change- A chemical change cannot be changed back to its original form. In a chemical change, bonds are broken and new bonds are formed between different atoms. This breaking and forming of bonds takes place when particles of the original materials collide with one another. Chemical Properties- Properties that describe how a substance changes into a completely different substance are called chemical properties. Flammability and corrosion/oxidation resistance are examples of chemical properties. Example: wood burning in a fire place. Bonding- Any of the interactions that account for the association of atoms into molecules, ions, crystals, metals, and other stable species. Covalent- Shares electrons- a chemical bond formed by the sharing of one or more electrons, especially pairs of electrons, between atoms. Ionic- gives away electrons- one or more electrons are transferred from one neutral atom (typically a metal)to another (typically a nonmetallic element Example: crystals of common salt (sodium chloride, NaCl) are dissolved in water, Metallic- sea of electrons- a chemical bond in which electrons are shared over many nuclei and electronic conduction occurs. Atomic Structure- The arrangement of the parts of an atom, which consists of a massive, positively charged nucleus surrounded by a cloud of electrons arranged in orbits. Atomic Theory- The physical theory of the structure, properties, and behavior of the atom Scientists and Models Democritus (Solid Spheres)- suggested in 450 BC that the “stuff” that makes up the world are composed of invisible particles. This theory has been disproved with the discovery of protons, electrons, neutrons, and even qwarks! Dalton (Billiard Ball)- performed many experiments and revised some of Democritus's ideas. He proposed his own atomic theory in 1803. The atoms of a given element are different from those of any other element; the atoms of different elements can be distinguished from one another by their respective relative atomic weights. All atoms of a given element are identical. Atoms of one element can combine with atoms of other elements to form chemical compounds; a given compound always has the same relative numbers of types of atoms. Atoms cannot be created, divided into smaller particles, nor destroyed in the chemical process; a chemical reaction simply changes the way atoms are grouped together. Elements are made of tiny particles called atoms. Thomson (Plum Pudding)- says that the eletrons are like raisins sitting in a plum pudding and the pudding is the rest of the atom is like the pudding. The rest of the atoms is positively charged to neutralized the negative charge of the electrons. Rutherford (Nuclear Atomic)- performed the Gold Foil Experiment and proved there was a positively charged nucleus in an atom surrounded by electrons but mostly empty space. In 1920 he changed his model to include protons (positively charged particles. Bohr (Planetary)- makes electrons look like planets revolving around the sun. In reality electrons move in different shapes and do not stay on the same path. Quantum Mechanical- also known as the Electron Cloud Theory. Scientists believe electrons fly in specific energy levels or shells around the nucleus. Acids and Bases Characteristics Acids- A substance that yields hydrogen ions when dissolved in water. A substance that can act as a proton donor. A substance that can accept a pair of electrons to form a covalent bond. Bases- A substance that can act as a proton acceptor. A substance that can donate a pair of electrons to form a covalent bond ACIDS BASES TASTE SOUR BITTER FEEL STINGS SLIPPERY REACTIONS YES / METAL CONDUCTS ELECTROLYTE RELEASES H+ NO / METALS ELECTROLYTE OH-