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Chapter 2: Chemical Units and Their Identities

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ATOMS: - made of nucleus (protons (positive charge) and neutrons (neutral charge)) and electron cloud (electrons (negative charge) - smallest particle that still retains properties of element - atomic # - # of protons (unique to each element) (also # of electrons in neutral atoms) - mass # - # of protons + neutrons - atomic mass - actual (average) mass of atom (measured in daltons) - about mass # b/c electrons have very small mass compared to protons/neutrons - isotope - atom w/ more/less than usual # of neutrons ELECTRONS: - elemental form of element is when element is by itself - compound - joint of 2+ elements w/ own set of properties diff. from elements - elements in periodic table are arranged in atomic # and are in 18 columns (groups)

Chapter 2

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AP Biology Reading Guide Chapter 2: The Chemical Context of Life Fred and Theresa Holtzclaw Copyright ? 2010 Pearson Education, Inc. - 1 - Name_______________________Period___________ Chapter 2: The Chemical Context of Life This chapter covers the basics that you may have learned in your chemistry class. Whether your teacher goes over this chapter, or assigns it for you do review on your own, the questions that follow should help you focus on the most important points. Concept 2.1 Matter consists of chemical elements in pure form and in combinations called compounds 1. Define and give an example of the following terms: matter element compound 2. What four elements make up 96% of all living matter?

What is a molecule?

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Molecule Main article: Molecule A molecule is the smallest indivisible portion of a pure chemical substance that has its unique set of chemical properties, that is, its potential to undergo a certain set of chemical reactions with other substances. Molecules can exist as electrically neutral units unlike ions. Molecules are typically a set of atoms bound together by covalent bonds, such that the structure is electrically neutral and all valence electrons are paired with other electrons either in bonds or in lone pairs.

Arrangement of Electrons in Atoms Vocabulary Terms

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Amplitude ? magnitude of change within an oscillating system of the oscillation variable with each oscillation Angular momentum quantum number ? the quantum number that indicates the shape of an orbital Atomic emission spectrum ? the range of the frequencies of electromagnetic radiation Aufbau Principle ? the principle that states that the structure of each successive element is obtained by adding one proton to the nucleus of the atom and one electron to the lowest-energy De Broglie?s Relation ? said that particles can exhibit wave-like behaviour Electromagnetic radiation ? the radiation associated with an electric and magnetic field. Varies periodically and travels at the speed of light Electromagnetic spectrum ?all of the frequencies or wavelengths of electromagnetic radiation

Electron configurations and Lewis dot structures quiz

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Name: Electron Configurations and Lewis Dot Structures Quiz Which is the correct ground state electron configuration for Fluorine? 1s22s22p5 1s22s22p2 1s22s22p4 1s22s22p1 Which is the correct ground state electron configuration for Neon? 1s22s22p63s1 1s22s22p5 1s22s22p43s1 1s22s22p6 The full electron configuration for an element is 1s22s22p63s1 . What element is this? What is this elements symbol on the periodic table How many valence electrons does this element have? Draw Lewis Dot Structures for the following elements C N O F Ne Si S P Cl Ar Based on the Lewis Dot Structures you drew in question 4 explain what relationship (if any) you notice between the group number and the number of valence electrons.

Electron filling diagram

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1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f ? 6s 6p 6d ? 7s 7p ? 8s ? The order of increasing energy of the sublevels: 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d ? This order corresponds to the order in which the energy sublevels are filled by electrons. nucleus 1s 2s 2p 3s 3p 4s 3d 4p 4d 4f n = 1 n = 2 n = 3 n = 4 Energy level (n) Energy sublevel Increasing Energy
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