Chapter 2 The Chemistry of Life. 2.1 The nature of matter

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1 Chapter 2 The Chemistry of Life 2.1 The nature of matter

2 Atoms make up all matter Composed of three parts: Protons, Neutrons, and Electrons Protons and Neutrons are found in the atom s neucleus Electrons are found in the space surrounding (orbiting) the neucleus

4 Each type of atom makes up a separate element Element a pure substance made up of only one type of atom. Represented by a 1 or 2 letter symbol. (EX: Oxygen=O, Sodium=Na)

5 Break it down The atomic number tells you the number of protons The number of protons is the same as the number of electrons ( THEY DO NOT ADD TOGETHER THEY ARE JUST THE SAME NUMBER). The atomic mass tells you the number of protons and neutrons which are added together.

6 Try These How Many (Protons, Neutrons, Electrons)?

7 Answers.. Sodium = 11 Protons (11 Electrons), 11 Neutrons (Atomic # 22 = Protons + Neutrons). Lithium = 3 Protons (3 electrons), 4 Neutrons (Atomic # 7 = Protons + Neutrons). Oxygen = 8 Protons (8 electrons), 8 Neutrons (Atomic # 16 = Protons + Neutrons).

8 Time for some math! Boron has 5 protons, and an atomic mass of 11. How many neutrons? How many electrons? Silicon has 14 protons and 14 neutrons. What is the atomic mass? How many electrons? Aluminum has 13 electrons and 14 neutrons. What is the atomic mass? How many protons?

9 Answers.. 6 neutrons, 5 electrons Atomic mass 28, 14 electrons 13 protons, Atomic mass 27

10 Isotopes Atoms of an element may have different numbers of neutrons. For example, although all atoms of carbon have six protons, some have six neutrons, some seven, and a few have eight. Atoms of the same element that differ in the number of neutrons they contain are known as isotopes.

11 The total number of protons and neutrons in the nucleus of an atom is called its mass number. Isotopes are identified by their mass numbers; for example, carbon-12, carbon-13, and carbon-14.

12 The weighted average of the masses of an element s isotopes, in which the abundance of each isotope in nature is considered, is called its atomic mass. Because they have the same number of electrons, all isotopes of an element have the same chemical properties.

13 Radioactive Isotopes Some isotopes are radioactive, meaning that their nuclei are unstable and break down at a constant rate over time. Although radiation can be dangerous, radioactive isotopes have a number of important scientific and practical uses. Geologists can determine the ages of rocks and fossils by analyzing the isotopes found in them. Radiation from certain isotopes can be used to detect and treat cancer and to kill bacteria that cause food to spoil. Radioactive isotopes can also be used as labels or tracers to follow the movements of substances within organisms.

two or more elements in definite proportions Represented by a

14 Atoms form bonds with each other to form molecules and compounds.. A compound is a substance formed by the chemical combination of two or more elements in definite proportions Represented by a chemical formula: (made of two hydrogen and one oxygen atom) is written as H 2 O

15 Two types of chemical bonds.. Ionic bonds: formed between oppositely charged ions

16 Covalent bonds: formed when two or more atoms share electrons

17 Van der Waals Forces Because of their structures, atoms of different elements do not all have the same ability to attract electrons. Some atoms have a stronger attraction for electrons than do other atoms. When the atoms in a covalent bond share electrons, the sharing is not always equal. Even when the sharing is equal, the rapid movement of electrons can create regions on a molecule that have a tiny positive or negative charge.

18 Van der Waals Forces When molecules are close together, a slight attraction can develop between the oppositely charged regions of nearby molecules. (think magnets) These intermolecular forces of attraction are called van der Waals forces. These forces are not as strong as ionic bonds or covalent bonds, but they can hold molecules together, especially when the molecules are large.

19 Chapter 2 The Chemistry of Life 2.2 Properties of Water

20 Water is vital to all organism because it has special properties Water is Polar Polarity characteristic of a molecule that involves and uneven distribution (sharing) of charges (has one or more positive end and negative end)

21 Water is polar because oxygen pulls more electrons towards itself so it has a slightly negative charge, leaving the hydrogen(s) with a slight positive charge

22 Polarity allows 3 properties: Adhesion H2O molecules stick to other polar molecules, but repel nonpolar molecules Cohesion H2O molecules stick to each other High Heat Capacity H2O can absorb a large amount of energy before its temperature increases, and holds energy longer than other substances

23 Water is used in many solutions. Solution a mixture in which all parts are evenly distributed, such as saltwater

24 Solute the part of a solution that is dissolved the salt in salt water Solvent the substance in a solution that dissolves the solute the water in salt water Water is the most common solvent because it can dissolve many things Often called the universal solvent

25 Acids, Bases, and ph Water molecules sometimes split apart to form hydrogen ions and hydroxide ions.

26 Acids, Bases, and ph In pure water, about 1 water molecule in 550 million splits to form ions in this way. Because the number of positive hydrogen ions produced is equal to the number of negative hydroxide ions produced, pure water is neutral.

27 The ph Scale Chemists devised a measurement system called the ph scale to indicate the concentration of H + ions in solution. The ph scale ranges from 0 to 14. At a ph of 7, the concentration of H + ions and OH ions is equal. Pure water has a ph of 7.

29 The ph Scale Solutions with a ph below 7 are called acidic because they have more H + ions than OH ions. The lower the ph, the greater the acidity. Solutions with a ph above 7 are called basic because they have more OH ions than H + ions. The higher the ph, the more basic the solution.

30 The ph Scale Each step on the ph scale represents a factor of 10. For example, a liter of a solution with a ph of 4 has 10 times as many H + ions as a liter of a solution with a ph of 5.

31 Acids An acid is any compound that forms H + ions in solution. Acidic solutions contain higher concentrations of H + ions than pure water and have ph values below 7. Strong acids tend to have ph values that range from 1 to 3. Hydrochloric acid (HCl) is a strong acid produced by the stomach to help digest food.

32 Bases A base is a compound that produces hydroxide (OH ) ions in solution. Basic, or alkaline, solutions contain lower concentrations of H + ions than pure water and have ph values above 7. Strong bases, such as the lye (commonly NaOH) used in soap making, tend to have ph values ranging from 11 to 14.

33 Buffers The ph of the fluids within most cells in the human body must generally be kept between 6.5 and 7.5 in order to maintain homeostasis. If the ph is lower or higher, it will affect the chemical reactions that take place within the cells. One of the ways that organisms control ph is through dissolved compounds called buffers, which are weak acids or bases that can react with strong acids or bases to prevent sharp, sudden changes in ph.

35 Buffers Adding acid to an un-buffered solution causes the ph of the un-buffered solution to drop. If the solution contains a buffer, however, adding the acid will cause only a slight change in ph.

Biology. Slide 1 of 40. End Show. Copyright Pearson Prentice Hall

Biology. Slide 1 of 40. End Show. Copyright Pearson Prentice Hall Biology 1 of 40 2-1 The Nature of Matter 2 of 40 2-1 The Nature of Matter Atoms Atoms The study of chemistry begins with the basic unit of matter, the atom. 3 of 40 2-1 The Nature of Matter Atoms Placed