2-1 The Nature of Matter

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1 2-1 The Nature of Matter

2 Small Atoms Placed side by side, 100 million atoms would make a row only about 1 centimeter long. contain subatomic particles

3 Atoms What three subatomic particles make up atoms?

4 The subatomic particles that make up atoms are protons neutrons electrons

5 The subatomic particles in a helium atom.

6 Protons and neutrons have about the same mass. Protons positively charged (+) Neutrons no charge. Strong forces bind protons and neutrons together form the nucleus at the center of the atom.

7 Electron negatively charged ( ) 1/1840 the mass of a proton. in constant motion in the space surrounding the nucleus.

8 are attracted to the positively charged nucleus remain outside the nucleus Because of the energy of their motion.

9 Atoms are neutral in charge have equal numbers of electrons and protons, have equal but opposite charges Proton +1 charge (P + ) Electron 1 charge (e - )

10 Elements and Isotopes Element pure substance that consists entirely of one type of atom. represented by a one- or two-letter symbol.» C stands for carbon.» Na stands for sodium.

11 atomic number The number of protons in an atom Carbon has 6 protons, so its atomic number is 6. More than 100 elements are known only about two dozen are commonly found in living organisms.

12 Isotopes Atoms of the same element Different number of mass number The sum of the protons and neutrons in the nucleus of an atom. Isotopes have different mass numbers

13 Isotopes are identified by their mass numbers. Example: carbon has three isotopes - each has a different number of neutrons carbon-12» C-12» 6 12 C carbon-13» C-12» 6 13 C carbon-14» C-14» 6 14 C

14 How are all of the isotopes of an element similar?

15 Because they have the same number of electrons, all isotopes of an element have the same chemical properties.

16 Isotopes of Carbon 6 electrons 6 protons 67 8 neutrons

17 Radioactive Isotopes Some isotopes are radioactive their nuclei are unstable and break down at a constant rate over time can be dangerous have important scientific and practical uses

18 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.

19 Chemical Compounds In nature, most elements are found combined with other elements in compounds. Compound a substance formed by the chemical combination of two or more elements in definite proportions. physical and chemical properties of a compound are different from the elements from which it is formed.

20 composition of compounds shown by formula Example Water H 2 O contains two atoms of hydrogen for each atom of oxygen. table salt (sodium chloride) NaCl sodium and chlorine combine in a 1 : 1 ratio.

21 What are the two main types of chemical bonds?

22 Chemical Bonds chemical bond Hold compounds together involves the electrons that surround each atomic nucleus.» The electrons that are available to form bonds are called valence electrons.

23 The main types of chemical bonds are: ionic bonds covalent bonds

24 Ionic Bonds ionic bond 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. Ions = positively and negatively charged atoms.

25 Sodium atom (Na) Sodium ion (Na+) Sodium ion (Cl - ) Sodium atom (Cl) Protons +11 Electrons Charge +1 0 Protons +17 Electrons Charge -10

26 Covalent Bonds electrons are shared by atoms instead of being transferred. the moving electrons actually travel in the orbitals of both atoms.

27 covalent bond when electrons are shared between atoms. When the atoms share two electrons the bond is called a single covalent bond. When atoms share four electrons The bond is called a double bond. When atoms share six electrons The bond is called a triple bond.

28 Molecule The structure that results when atoms are joined together by covalent bonds. the smallest unit of most compounds.

29 In a water molecule, each hydrogen atom forms a single covalent bond with the oxygen atom.

30 Van der Waals Forces When molecules are close together slight attraction can develop between the oppositely charged regions of nearby molecules. such intermolecular forces of attraction are called van der Waals forces. not as strong as ionic bonds or covalent bonds can hold molecules together» especially when the molecules are large.

31 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.

32 1. The particles that move around the nucleus of an atom are called A. neutrons. B. protons. C. electrons. D. isotopes.

33 2. 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

34 3. 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.

35 4. 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.

36 5. 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.

37 END

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