Integrated Coordinated Science End of Year Review

Part 3: Chemistry

Atomic and Molecular Structure Standard 1a: Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass. An atom consists of a nucleus made of protons and neutrons that is orbited by electrons. Number of protons, not electrons or neutrons, determines the unique properties of an element. e - e-e- p+p+ n p+p+

Atomic and Molecular Structure Standard 1a: Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass. Elements are arranged on the periodic table in order of increasing atomic number from left to right. This number of protons is called the atomic number. C Atomic number

Atomic and Molecular Structure Standard 1a: Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass. If elements were ordered by atomic mass, this would lead to misplaced elements due to differences in number of neutrons for isotopes of the same element affect the atomic mass but do not change the identity of the element.

Standard 1b: Students know how to use the periodic table to identify metals, semimetals, non-metals, and halogens. Atomic and Molecular Structure Halogens

Standard 1c: Students know how to use the periodic table to identify alkali metals, alkaline earth metals and transition metals, trends in ionization energy, electronegativity, and the relative sizes of ions and atoms. Atomic and Molecular Structure Electronegativity is a measure of the ability of an atom of an element to attract electrons toward itself in a chemical bond using range from 0 (no attractiveness) to 4.0 (highest attractiveness).

Standard 1c: Students know how to use the periodic table to identify alkali metals, alkaline earth metals and transition metals, trends in ionization energy, electronegativity, and the relative sizes of ions and atoms. Atomic and Molecular Structure Ionization energy is the energy it takes to remove an electron from an atom.

Standard 1c: Students know how to use the periodic table to identify alkali metals, alkaline earth metals and transition metals, trends in ionization energy, electronegativity, and the relative sizes of ions and atoms. Atomic and Molecular Structure Generally in the periodic table, ionization energy and electronegativity increase from left to right because of increasing numbers of protons and decrease from top to bottom owing to an increasing distance between electrons and the nucleus.

Standard 1c: Students know how to use the periodic table to identify alkali metals, alkaline earth metals and transition metals, trends in ionization energy, electronegativity, and the relative sizes of ions and atoms. Atomic and Molecular Structure Atomic and ionic sizes generally decrease from left to right and increase from top to bottom for the same reasons.

Atomic and Molecular Structure Standard 1d: Students know how to use the periodic table to determine the number of electrons available for bonding. Only electrons in the outermost energy levels of the atom are available for bonding; this outermost bundle of energy levels is often referred to as the valence shell or valence shell of orbitals. All the elements in a group have the same number of valence electrons in their outermost energy level or

Atomic and Molecular Structure Standard 1e: Students know the nucleus of the atom is much smaller than the atom yet contains most of its mass. The mass of the atom is densely packed in the nucleus in the form of protons and neutrons. An atom is made up of the nucleus (protons and neutrons) and electron cloud combined.

Atomic and Molecular Structure Standard 1e: Students know the nucleus of the atom is much smaller than the atom yet contains most of its mass. The electrons occupy a large region of space centered around a tiny nucleus, and so it is this region that defines the volume of the atom. The electron is almost 2,000 times lighter than the proton; therefore, the large region of space occupied by the electron contains less than 0.1% of the mass of the atom.

Chemical Bonds Standard 2a: Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds. If atoms want to keep their valence electrons, they will share them in one of two types of bonds: OO C 1. Covalent bond: bond in which non-metals share electrons between them

Chemical Bonds Standard 2a: Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds. Al If one atom wants to lose its valence electrons while the other atom wants to keep its valence electrons, they will exchange or transfer them in an ionic bond. Na Cl 2. Metallic bond: bond in which metals share electrons between them in a loose lattice Al

Chemical Bonds Standard 2b: Students know chemical bonds between atoms in molecules such as H 2, CH 4, NH 3, H 2 CCH 2, N 2, Cl 2, and many large biological molecules are covalent. If atoms are both non-metals, they will be covalent (share electrons). Many molecules like hydrogen (H 2 ), methane (CH 4 ), ammonia (NH 3 ), ethylene gas (C 2 H 4 ), nitrogen (N 2 ), and chlorine (Cl 2 ) are covalent. H2H2 CH 4 NH 3 N2N2 Cl 2 C2H4C2H4

Chemical Bonds Standard 2c: Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction. Salt: A chemical compound formed when a cation (positive charge) bonds with an anion (negative charge) Example is when sodium (Na +1 ) combines with chlorine (Cl -1 ) to form table salt

Chemical Bonds Standard 2c: Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction. Repeating patterns of positive and negative ions form crystals Salt crystals are held together by ionic bonds, which are formed because of the attraction between opposite charges, or electrostatic attraction.

Acids and Bases Standard 5a: Students know the observable properties of acids, bases, and salt solutions. Acid Tastes sour Feels watery Conducts electricity Corrosive/damaging turns litmus red pH < 7.0 React with metals to produce H 2 gas Neutralizes bases Acid: substance that produces hydrogen ions (H + ) in solution

Acids and Bases Standard 5a: Students know the observable properties of acids, bases, and salt solutions. Base Tastes bitter Feels slippery Conducts electricity Corrosive/damaging Turn litmus blue pH > 7.0 Do NOT react with metals Neutralizes acids Base: substance that produces hydroxide ions (OH - ) in solution

Acids and Bases Standard 5a: Students know the observable properties of acids, bases, and salt solutions. Salt Solution Taste salty Feel watery Water and salt acidic, basic or neutral May be neutral Salt solution: a crystalline compound formed from the neutralization of an acid by a base containing a metal

Acids and Bases Standard 5c: Students know strong acids and bases fully dissociate and weak acids and bases partially dissociate. An acid fully dissociates when all of the H + ions separate from the compound. A base fully dissociates when all of the OH - ions separate from the compound.

Acids and Bases Standard 5c: Students know strong acids and bases fully dissociate and weak acids and bases partially dissociate. Strong acids or bases will fully dissociate. Weak acids or bases will partially dissociate.

Chemical Thermodynamics Standard 7b: Students know chemical processes can either release (exothermic) or absorb (endothermic) thermal energy. Chemical reactions involve transfer of energy as heat. This is called chemical thermodynamics. Thermodynamic reactions in which energy is lost or released are called exothermic reactions. Energy Exits = Exothermic

Chemical Thermodynamics Standard 7b: Students know chemical processes can either release (exothermic) or absorb (endothermic) thermal energy. Thermodynamic reactions in which energy is gained or absorbed are called endothermic reactions. Energy Enters = Endothermic

Chemical Thermodynamics Standard 7c: Students know energy is released when a material condenses or freezes and is absorbed when a material evaporates or melts. CONDENSATIONFREEZING MELTINGEVAPORATION liquid solid gas When chemicals condense or freeze, energy is released (to make it colder). Energy released/exits = exothermic Energy absorbed/enters = endothermic When chemicals melt or evaporate, energy is absorbed (to heat it up).

End of Part 3: Chemistry