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Introduction to Chemistry: Matter and its Interactions

Introduction to Chemistry: Matter and its Interactions. Mr. Pierson Fall 2013. Atoms . Consist of protons , neutrons , and electrons Protons – positively charged subatomic particle found in the nucleus Electrons – negatively charged subatomic particle outside of the nucleus

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Introduction to Chemistry: Matter and its Interactions

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  1. Introduction to Chemistry: Matter and its Interactions Mr. Pierson Fall 2013

  2. Atoms • Consist of protons, neutrons, and electrons • Protons – positively charged subatomic particle found in the nucleus • Electrons – negatively charged subatomic particle outside of the nucleus • Neutrons – neutrally charged (no charge) subatomic particle found in the nucleus

  3. The Periodic Table • Elements – simplest forms of matterthat can exist under normal laboratory conditions. • Matter – anything that takes up space and has mass. • Mass– the amount of matter that an object contains. • The periodic table orders elements horizontally by the number of protons in the atom’s nucleus and places those with similar chemical properties in columns. • Chemical property – the ability of a substance to undergo chemical reactions and to form new substances.

  4. Important Things to Learn Right Away • Symbols of Common Elements • Symbols of Common Polyatomic Ions • The Periodic Table • Alkali metals • Alkaline earth metals • Nonmetals • Noble gases

  5. The Alkali Metals • Li • Na • K • Rb • Cs • Fr

  6. Alkaline Earth Metals • Be • Mg • Ca • Sr • Ba • Ra

  7. Nonmetals • B • C, Si • N, P, As • O, S, Se, Te • F, Cl, Br, I, At

  8. Noble Gases • He • Ne • Ar • Kr • Xe • Rn

  9. Metals, Nonmetals, Metalloids • Metals – elements that have a high electrical conductivity and a high luster when clean. • Nonmetals – elements that are nonlustrous and are generally poor conductors of electricity. • Example: Argon, Chlorine (gases); Carbon, Sulfur (solids); Bromine (liquid at room temp.) • Metalloids – elements with the properties of both metals and nonmetals. • Example: Silicon and Germanium

  10. Assignment • Pg. 109, “Concept Practice” #1 • Pg. 136, “Practice Questions and Problems” #32 • Pg. 137, “Mastery Questions and Problems” #54 • List the symbol and names of the Alkali Metals, Alkaline Earth Metals, Nonmetals, and Noble Gases

  11. Atoms and Ions • Ions- atoms or groups of atoms that have a positive or negative charge. • Cations – any atom or group of atoms with a positive charge • Has less electrons than protons • Example: Na+ • Has 11 protons and only 10 electrons when it loses an electron (with 1 more proton only the “+” is used, if 2 more protons than electrons we would write “2+” to represent that there are 2 more protons than electrons) • Anions – atoms or groups of atoms with a negative charge • Has more electrons than protons • Example: Cl- • Has 17 protons and 18 electrons when chlorine gains an electron. Remember, electrons are negatively charged, so in this case we have 18 negatives and 17 positives for an overall -1 (17-18).

  12. Compounds • Molecule – an electrically neutral group of atoms that act as a unit. • Example: H2O • Water is a molecular compound – compounds that are composed of molecules • Ionic Compound – composed of positive cations and negative anions. • Example: NaCl • Chemical formula – shows the number and kinds of atoms in the smallest representative unit of the substance. • Molecular formula – shows the number and kinds of atoms present in a molecule of a compound.

  13. Compounds, cont. • Chemical compound (compound = 2 or more things combined) • Molecular (2 or more molecules) • Ionic (2 or more ions) • All different compounds have different properties • Must use chemical formula (remember, a chemical symbol is the same thing as an element symbol, i.e. H, He, etc.) • If the chemical is a molecular compound, then a molecular formula is used • Example: H2O

  14. Formula Units • = the lowest whole-number ratio of ions in an ionic compound. • Example: Sodium Chloride • Na+ needs 1 electron and Cl- has 1 extra electron, the ratio is 1:1, thus the formula unit is NaCl. • Mg2+ needs 2 electrons and Cl- has 1 extra electron, so it would take 2 Cl- anions to combine with the Mg2+ cation, thus the ratio is 1:2 and the formula unit = MgCl2 • What would the formula unit be for Li+ and S2- ions?

  15. In-Class Assignment • Read pg. 116 – 123 • Copy Table 5.4 “Common Polyatomic Ions” into your notes.

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