Biology Slide 1 of 40 Copyright Pearson Prentice
Biology Slide 1 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Slide 2 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Atoms *The study of chemistry begins with the basic unit of matter, the atom. The Greek philosopher Democritus called the smallest fragment of matter the atom, from the Greek word atomos. Slide 3 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Atoms contain subatomic particles that are even smaller. Slide 4 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Atoms What three subatomic particles make up atoms? Slide 5 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Atoms The subatomic particles that make up atoms are • Protons- (+) positive charge • Neutrons- (0) no charge neutral • Electrons- (-) negative charge Slide 6 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Atoms The subatomic particles in a helium atom. Slide 7 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Atoms Protons and neutrons are found in the nucleus or center of the atom. They are held together by strong forces. Protons & neutrons have about the same atomic mass, which is 1. *The atomic mass is the total number of protons & neutrons. Slide 8 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Atoms * Electrons are in constant motion in the space surrounding the nucleus. *They have a negligible atomic mass (0). Electrons are attracted to the positively charged nucleus but remain outside the nucleus because of the energy of their motion. Slide 9 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Atoms Slide 10 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Atoms *Because atoms have equal numbers of electrons and protons, and because these subatomic particles have equal but opposite charges, atoms are neutral. *protons (+) = electrons (-) If an atom has a charge it is called an Ion. * + ion- protons > electrons * - ion- protons< electrons Slide 11 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Elements and Isotopes A chemical element is a pure substance that consists entirely of one type of atom. *Elements are represented by a one- or two-letter symbol. • Ex: C stands for carbon. • Ex: Na stands for sodium. Slide 12 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Elements and Isotopes *The number of protons in an atom of an element is the element's atomic number (symbol Z). Carbon has 6 protons, so its atomic number is 6. *Every element has its own atomic number so it identifies the element. More than 100 elements are known, but only about two dozen are commonly found in living organisms. Slide 13 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Rules: 1. To find Protons, it is the same as the atomic number. 2. Protons = Electrons 3. To find Neutrons: atomic mass – atomic number Slide 14 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter *Periodic Table – list of all the elements Symbols- for the names of the elements Atomic numbers Atomic mass 6 atomic number C symbol atomic mass 12. 01 Slide 15 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Elements and Isotopes Def: Atoms of the same element that differ in the number of neutrons they contain are known as isotopes. Slide 16 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Elements and Isotopes *Isotopes are identified by their mass numbers. For example, carbon has three isotopes—carbon-12, carbon-13, and carbon-14. Each isotope has a different number of neutrons. Slide 17 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Elements and Isotopes How are all of the isotopes of an element similar? Slide 18 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Elements and Isotopes Because they have the same number of electrons, all isotopes of an element have the same chemical properties. Slide 19 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Elements and Isotopes of Carbon 6 electrons 6 protons 6 neutrons 7 neutrons 8 neutrons Copyright Pearson Prentice Hall Slide 20 of 40
2 -1 The Nature of Matter Elements and Isotopes Radioactive Isotopes Def: Some isotopes are radioactive, meaning that their nuclei are unstable and break down at a constant rate over time. Although the radiation these isotopes give off can be dangerous, they have important scientific and practical uses. Slide 21 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Elements and Isotopes *Radioactive isotopes can be used: • to determine the ages of rocks and fossils. • to treat cancer. • to kill bacteria that cause food to spoil. • as labels or “tracers” to follow the movement of substances within an organism. Slide 22 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Compounds In nature, most elements are found combined with other elements in compounds. Def: A chemical compound is a substance formed by the chemical combination of two or more elements in definite proportions. *The physical and chemical properties of a compound are different from the elements from which it is formed. Slide 23 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Compounds *Scientists show the composition of compounds by a kind of shorthand known as a chemical formula. Ex: Water, H 2 O, contains two atoms of hydrogen for each atom of oxygen. Ex: The formula for table salt, Na. Cl, indicates that sodium and chlorine combine in a 1 : 1 ratio. *When no subscript is present, 1 is understood. Slide 24 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds What are the two main types of chemical bonds? Slide 25 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds Def: The atoms in compounds are held together by chemical bonds. *Bond formation involves the electrons that surround each atomic nucleus. These are called Valence electrons. Slide 26 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds The main types of chemical bonds are: • ionic bonds • covalent bonds Slide 27 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds Ionic Bonds Def: An ionic bond is formed when one or more electrons are transferred from one atom to another. *An atom that loses electrons has a positive charge. *An atom that gains electrons has a negative charge. These positively and negatively charged atoms are known as ions. Slide 28 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Sodium atom (Na) Sodium ion (Na+) Chemical Bonds Chlorine atom (Cl) Chloride ion (Cl-) Protons +11 Electrons - 10 Protons +17 Electrons - 18 Electrons - 17 Charge 0 Charge +1 Charge -1 Charge 0 Slide 29 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds Covalent Bonds *Sometimes electrons are shared by atoms instead of being transferred. Sharing electrons means that the moving electrons actually travel in the orbitals of both atoms. Slide 30 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds A covalent bond forms when electrons are shared between atoms. • 1 When the atoms share two electrons, the bond is called a single covalent bond. Ex: C-C • 2 When atoms share four electrons it is called a double bond. Ex: C C • 3 When atoms share six electrons it is called a triple bond. Ex: C C Slide 31 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds Def: The structure that results when atoms are joined together by covalent bonds is called a molecule. *A molecule is the smallest unit of most compounds. Slide 32 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds In a water molecule, each hydrogen atom forms a single covalent bond with the oxygen atom. Slide 33 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds Van der Waals Forces *When molecules are close together, a slight attraction can develop between the oppositely charged regions of nearby molecules. Chemists call such intermolecular forces of attraction van der Waals forces, after the scientist who discovered them. Slide 34 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds Although van der Waals forces are not as strong as ionic bonds or covalent bonds, they can hold molecules together, especially when the molecules are large. Slide 35 of 40 Copyright Pearson Prentice Hall
2 -1 The Nature of Matter Chemical Bonds *For example, van der Waals forces form between the molecules on the surface of a gecko’s foot and the molecules on the surface of the wall. The combined strength of all the van der Waals forces allows the gecko to grip the wall. Slide 36 of 40 Copyright Pearson Prentice Hall
2 -1 Click to Launch: Continue to: - or - Slide 37 of 40 Copyright Pearson Prentice Hall
2 -1 The particles that move around the nucleus of an atom are called a. neutrons. b. protons. c. electrons. d. isotopes. Slide 38 of 40 Copyright Pearson Prentice Hall
2 -1 The atomic number of a carbon atom is 6. How many neutrons does the isotope carbon-14 have? a. 6 b. 8 c. 12 d. 14 Slide 39 of 40 Copyright Pearson Prentice Hall
2 -1 Which of the following statements about the three isotopes of carbon is true? a. They are all radioactive. b. They have different numbers of electrons. c. They have the same chemical properties but differ in atomic mass. d. They have the same number of protons and neutrons. Slide 40 of 40 Copyright Pearson Prentice Hall
2 -1 A chemical compound consists of a. electrons mixed with neutrons. b. two or more elements combined in a definite proportion. c. two or more elements combined in any proportion. d. at least three elements combined by ionic or covalent bonds. Slide 41 of 40 Copyright Pearson Prentice Hall
2 -1 Van der Waals forces are the result of a. unequal sharing of electrons. b. ionic bonds. c. the bonding of different isotopes. d. the chemical combination of sodium and chlorine. Slide 42 of 40 Copyright Pearson Prentice Hall
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