Name: Class key. Period: Chapter 6 Basic Chemistry assignments. The Living Environment 14-15
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1 Name: Class key Period: Chapter 6 Basic Chemistry assignments
2 Pages/Sections Date Assigned Date Due
3
4 Topic: Atoms and Elements Objective: Compare and/or contrast atoms and elements. Atoms o atoms are the basic building blocks of matter. cannot be divided by chemical means. Elements o substance made entirely from one type of atom. Just over 100 elements ( 100+ different atoms).
5 Topic: Elements & Compounds Objective: Compare and/or contrast elements and compounds. Compounds (Slide 1) o two (or more ) elements combined in definite proportions. water H 2 0: 2 hydrogen atoms; 1 oxygen atom.
6 Topic: Atomic Structure Objective: Describe the structure of individual atoms. Each atom has: o nucleus central core (Slide 2) neutrons (except H) neutral. protons (p + ) and neutrons (n 0 ) have same mass. (Slide 3) nucleus is chemically stable ; does not normally change. Electrons surround nucleus; negligible mass.
7 Notes page:
8 Topic: Atoms - Names & Numbers Objective: Describe atomic and mass numbers for elements. protons positive charge; _determines the atomic number. Add protons and neutrons for mass number. (Slide 4)
9 Topic: Atoms Electron Shells Objective: Describe electron shells and energy levels. Shell outer ring o contains at least negatively charged 1 e - ( electron ). o electron is considered to have negligible (insignificant) mass. o Energy levels ( shells ) hydrogen is only element with unfilled first shell. helium has first filled 2 e - shell. lithium starts with second level (max 8 e - ). (Slide 5)
10 Topic: Atoms Isotopes Objective: Describe atomic isotopes and numbering. Isotopes o isotopes Atoms that vary their number of neutrons. number of protons does not change ( same atomic number= same element name ). mass number (# of neutrons ) changes. written with small superscript isotope number to upper left 18 O. (Slide 6)
11 Topic: Atoms Radioactivity Objective: Describe radioactive isotopes and numbering. _Radioactive_ isotopes (_radioisotopes_). o unstable nucleus gives off ( emits ) charged particles. changes number of protons (atomic number) or neutrons (mass number). Process called radioactivity. Can be used to treat cancers (directed at cancer cells). Can be used as tags to trace compounds in a body; tags picked up by x-ray machines.
12 Notes page:
13 Name: Period: Carefully remove this sheet from your packet to hand in. Work silently and alone to complete this graded exercise. Check for Understanding 1. Describe the difference between an atom and an element. a. 2. What will adding a proton to an atom change? a. 3. Where are electrons located in an atom? a. 4. Is all radioactivity harmful? Explain. a.
14 Page intentionally blank
15 Topic: Chemical Bonding Objective: Describe covalent and ionic bonds. Chemical Bonding & Chemical Reactions. o Two major types of bonding ( joining ) of two (or more) atoms into a new structural compound. 1. covalent bonding. 2. ionic bonding.
16 Topic: Covalent Bonding Objective: Describe covalent bonds. Covalent Bonds. o molecule two or more atoms combined and act chemically as a single particle. o shared electrons ( electrons shared by molecules ) between two atoms has force. force is called chemical (covalent) bonding. H 2 O is polar covalent (shared) bond. (Slide 7) diatomic molecule is special covalent bond of two identical atoms. (Slide 8)
17 o e - always wants to fill outermost most energy levels. Can work with 2, 3, or 4 atoms.
18 Topic: Ionic Bonding Objective: Describe ionic bonds. Ionic bonds. o Only works with two atoms; forms ions. o e - is transfered from one with least to one with most. o Resultant ion is charged positive or negative. e.g. Na + and Cl - o Doesn t form multi-element molecules; forms two - atom type crystal easier to break. (Slide 9)
19
20 Topic: Covalent vs. Ionic bonds Objective: Compare/contrast covalent and ionic bonds. Comparison (Slide 10) shared electron in covalent bond forms a stronger bond ( higher energy value ). Electron given up in ionic bond forms a weaker bond ( lower energy value ). Notes page:
21
22 Topic: Chemical Reactions Objective: Describe chemical reactions, reactants, & products. Chemical Reactions o Compound certain elements bonded in definite proportions ( ratios ). Chemical reaction when forming different substances. (Slide 11) o Reaction requires some energy to be input ; may result in more energy being released than was input. o Reactants = original substances. o products = new substances.
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24 Topic: Conservation of Mass Objective: What happens to the matter (mass) in reactions? Law of conservation of mass = reactant s mass must equal product s mass. Creates a balanced equation = numbers of reactant atoms equals numbers of product atoms formed. (Slide 12) Energy used absorbed and/or created released _is_ from e - _attractions_ in _bonds_ and won t change mass.
25 Topic: Chemical Formulas Objective: Describe the types of chemical formulas. Formulas (Slide 13) o Chemical ( molecular ) formula shows each atom & how many. o structural formula shows number, type, and how bonded ( shape ). o 3-D formulas model actual relationships between individual atoms.
26 Notes page:
27 Name: Period: Carefully remove this sheet from your packet to hand in. Work silently and alone to complete this graded exercise. Check for Understanding 1. Describe chemical bonding in your own words. a. 2. Compare and/or contrast both covalent and ionic bonding. a. 3. What is required for chemical reactions? a. 4. Describe what chemical formulas provide. (Answer on back)
28 a.
29 Notes page:
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