CHM 111 Lecture Notes - Lecture 4: Polyatomic Ion, Molar Mass, Periodic Trends

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7 Oct 2018

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CHM 111 Lecture Notes - Lecture 3: Unified Atomic Mass Unit, Microsoft Powerpoint

CHM 111 Lecture Notes - Lecture 4: Polyatomic Ion, Molar Mass, Periodic Trends

CHM 111 Lecture Notes - Lecture 5: Microsoft Powerpoint, Ionic Compound, Sulfite

Document Summary

Atoms at start of reaction will be there at end of reaction (balanced) Electrons can transfer from one atom to the other. Ion: atom(s) with a positive or negative charge. When a neutral atom loses one or more electrons. Formed by metals: anion: negatively charged ion. When a neutral atom gains one or more electrons. Formed by nonmetals: monatomic ion: ion with one atom, polyatomic ion: ion with more than one atom. Mendeleev: elements are orders by their atomic mass, elements with similar properties are in the same column, periodic law arranges the elements by atomic mass. Metals: solid at room temperature (except for hg, conducts heat and electricity, loses electrons in reactions (cations, malleable, ductile, 75% of elements are metals. Nonmetals: poor conductors of heat and electricity, gains electrons in reactions (anions, solids are brittle. Metalloids: aka semiconductors, have properties of metals and nonmetals. Atomic mass: the average mass of an element.

Related Questions

1. True or False. a. A positively charged ion is called an anion. b. If an atom gives up an electron, it creates negatively charged ion. c. Valence electrons are the electrons that are available for bonding and located in the shells closest to the nucleus. d. An ionic bond is the result of electron sharing. e. When atoms gain, lose, or share electrons they do so in order to have an electron configuration of a noble gas. f. As you go across the periodic table left to right, electronegativity will increase. g. The number of valence electrons an atom has is equal to the atomic number. h. Fluorine cannot be the central atom due to the fact that is can only accept 2 electrons. i. When a covalent bond occurs, the atoms overlap one another to create a new orbital. The more overlapping, the stronger the bond. j. A triple bond is considered to be a weak bond.

Predict the charge that an aluminum ion would have.