1. Chemistry

2. Structure of an Atom Protons and an Atoms identity Valence Electrons and Reactivity The Periodic Table Chemical Formulas Chemical Reactions Chemical Equations Law of Conservation of Mass Chemistry Unit 1 Chemistry Unit 2

3. Teks for Unit 1 and 2 (5) Matter and energy. The student knows that matter is composed of atoms and has chemical and physical properties. The student is expected to: Unit 1 (A) describe the structure of atoms, including the masses, electrical charges, and locations, of protons and neutrons in the nucleus and electrons in the electron cloud; (B) identify that protons determine an element's identity and valence electrons determine its chemical properties, including reactivity; (C) interpret the arrangement of the Periodic Table, including groups and periods, to explain how properties are used to classify elements; Unit 2 (D) recognize that chemical formulas are used to identify substances and determine the number of atoms of each element in chemical formulas containing subscripts; (E) investigate how evidence of chemical reactions indicate that new substances with different properties are formed; and (F) recognize whether a chemical equation containing coefficients is balanced or not and how that relates to the law of conservation of mass.

4. Chemistry Vocabulary, Unit 1, part 1 atom: the smallest particle of an element that has all the properties of that element element: a pure substance, made up of similar atoms, that cannot be broken down by chemical means nucleus: the center of an atom, which contains protons and neutrons proton: the subatomic particle in the nucleus that has a positive electric charge neutron: the subatomic particle in the nucleus that has no electric charge electron cloud: the region around the nucleus where electrons are found electron: the negatively charged subatomic particle that exists in a cloud surrounding the nucleus unified atomic mass unit (u): the unit for measuring the mass of atoms electric charge: a property of matter that causes it to experience a force near other charged matter valence electrons: the outermost electrons of an atom, which help determine an element’s chemical properties ion: an atom or molecule that has gained or lost one or more electrons chemical bond: an attractive force between atoms or ions, formed by the sharing or transfer of valence electrons Periodic Table: a logical arrangement of the elements into rows and columns; an element’s position in the Periodic Table can be used to predict its properties

5. Protons Neutrons Electrons Protons, Neutrons and Electrons AtomsMoleculesMineralsRocksEarth Mineral The Hierarchical Relationship of Atomic Structure

6. Element A pure substance, made up of similar atoms, that cannot be broken down by chemical means An element’s identity is determined by the number of protons. Interactive Periodic Table http://www.ptable.com/ http://www.ptable.com/

7. Meet the Elements Meet the Elements Video

8. What do you know about atoms? Atom

9. Components of an Atom Proton Neutron Electron All about Atoms

10. Nucleus Nucleus is a term used to describe the control center in an animal cell (Biology) Nucleus is the term to describe the very dense region at the center of an atom (Chemistry) Is this an animal or a plant cell?

11. Protons Have a positive charge Mass =1u or 1amu (unified atomic mass) Located in the nucleus The number of protons determines the elements identity Captain Proton A proton is made up of two up quarks and one down quark

12. Neutrons Neutral Charge Mass 1u Located in the Nucleus Elements with a variable number of neutrons are called isotopes

13. APE MAN Atomic Number = #Protons = #Electrons Mass Number- Atomic Number = Neutrons

15. Electrons and the Electron Cloud Electron Mass: Close to 0 u Electrons have a Negative Charge Electrons are located in the Electron Cloud Atoms with a different number of electrons are called ions. The Electrons cloud is subdivided into shells The shells hold a fixed amount of electrons – 1 st shell holds 2 electrons – 2 nd shell holds 8 electrons – 3 rd shell holds 8 electrons

16. The formation of Salt

17. Nucleus 1 2 3 4 5 Shell 1 holds 2 electrons Shell 2 holds 8 electrons Shell 3 holds 8 electrons Shell 4 holds 18 electrons Shell 5 holds 18 electrons 1 2 3 4 5

19. Atomic Components Atomic ParticleElectrical ChargeMassLocation in Atom Proton+1 uNucleus Neutronneutral1 uNucleus Electron-0 uElectron Cloud different element If the number of protons change, you have a different element. isotope If the number of neutrons change, you have an isotope. ion If the number of electrons change, you have an ion.

20. Opposite charges attract, whereas like charges repel

21. Valence Electrons Valence Electrons determine an elements chemical properties, including reactivity. Valence Electrons refer to the number of electrons in their outer shell

22. Lewis Dot Structure Ne H He Si O C B Be Li

23. Lewis Dot Structure

25. Chemistry Vocabulary, Unit 1, Part 2 Periodic Table: a logical arrangement of the elements into rows and columns; an element’s position in the Periodic Table can be used to predict its properties group: a column of the Periodic Table; elements in the same group have similar properties period: a row of the Periodic Table valence electrons: the outermost electrons of an atom, which help determine an element’s chemical properties metal: an element that is typically dense, shiny, strong, and a good conductor of heat and electricity nonmetal: an element that typically is not dense, and is dull, brittle, and a poor conductor of heat and electricity metalloid: an element that has properties between those of a metal and nonmetal; also called a semimetal pure substance: matter that has the same chemical composition throughout compound: a substance that forms when two or more elements join chemically molecule: a group of two or more atoms held together by chemical bonds chemical formula: a group of chemical symbols and numbers that shows the kinds and numbers of atoms in a molecule

27. Glue Nows!

30. Shell 1 holds 2 electrons Shell 2 holds 8 electrons Shell 3 holds 8 electrons Shell 4 holds 18 electrons Nucleus 1 2 3 4 5 1 2 3 4 5

31. Atomic Structure 1. Of the 10 atoms you modeled, which 2 are the most stable? Explain. 2. Look at the electron structures for lithium and fluorine. In a chemical reaction, the valence electron of a lithium atom transfers to the fluorine atom. This changes both atoms into ions. Explain why this reaction occurs. 3. When hydrogen and oxygen react, they combine in a 2-to-1 ratio to form a molecule of water (H 2 O). In this reaction, each of the 2 hydrogen atoms shares its valence electron with 1 oxygen atom. Explain why this reaction takes place in terms of the number of valence electrons. As you answer these questions, remember that atoms tend to be most stable when their outer energy level is full with electrons. They gain, lose, or share their outer electrons— called valence electrons—to achieve a full outer set.

32. Atomic Particle Electrical Charge MassLocation in Atom Atomic Particle Electrical Charge MassLocation in Atom Atomic Particle Electrical Charge MassLocation in Atom

33. 8. a Key Concepts An atom is the basic component of matter. All the atoms of a specific element, such as hydrogen, are similar. Elements are the basic substances or building blocks that make other substances. For example, the elements hydrogen and oxygen combine to form water. The elements sodium and chlorine combine to form table salt. The center of an atom is called the nucleus. The nucleus contains smaller particles called protons and neutrons. The electron cloud contains electrons that surround the nucleus. The electrons can be found anywhere in the cloud, but are more likely to be found in some places than in others. The mass of the particles of an atom are recorded in unified atomic mass units (u). The mass of each proton and neutron is very close to 1 u. Electrons have almost no mass. Some atoms in an element can have different numbers of neutrons. Because of this, the average atomic mass of the atoms for that element is used to describe atoms. For example, about 99 percent of carbon atoms in nature have a mass of 12 u. About 1 percent of carbon atoms have a mass of about 13 u. To find the average, perform the following calculation: 0.99 x 12 u + 0.01 x 13 u = 12.01 u The average mass of a carbon is about 12.01 u. Protons and electrons have electric charge. Opposite charges attract, whereas like charges repel. The proton has a positive charge, and the electron has a negative charge. The neutron does not have a charge.

34. 8.5 B Scientists have identified over 100 elements. Each element is made of a characteristic type of atom. All atoms contain a central core called the nucleus. The nucleus contains one or more protons, which are positively charged particles. Most nuclei also contain neutrons, which are uncharged particles. Neutrons help keep the nucleus from breaking apart. Surrounding the nucleus are fast-moving electrons, which are very small, negatively charged particles. The identity of an element is determined by the number of protons in the atomic nucleus. For example, every helium atom has two protons in its nucleus. Every oxygen atom has eight protons. The number of protons per atom is called the atomic number of the element. Helium has an atomic number of 2. Oxygen has an atomic number of 8. Atoms of the same element may have different numbers of neutrons in their nuclei. Most helium atoms have two neutrons, but some have only one neutron. Every atom is electrically neutral. Protons carry the positive charge of the atom, and electrons carry the negative charge. The number of protons equals the number of electrons. Electrons are organized into energy levels. The first energy level is filled with two electrons, and the second energy level is filled with eight electrons. For the first 20 elements, eight electrons also fill the third energy level. The diagram shows the first three elements that have full energy levels: helium, neon, and argon. The electrons in an atom’s outer energy level are called valence electrons. Atoms tend to be most stable when they have filled outermost energy levels. To reach this stability, atoms gain, lose, or share valence electrons by forming chemical bonds with other atoms.

35. Questions? The atomic number of oxygen is 8. What do all oxygen atoms have in common? How many possible electrons are in the first and second energy levels? What are valence electrons? How do valence electrons affect the chemical properties of an element? Describe the chemical reaction that occurs between sodium, whose atoms have 1 valence electron, and chlorine, whose atoms have 7 valence electrons

36. 8.5C The Periodic Table arranges elements in rows, called periods, and columns, called groups. The order of the elements is determined by atomic number. The periods grow in size on the table from top to bottom. The first period has only two elements, hydrogen (atomic number 1) and helium (atomic number 2). The second and third periods each contain eight elements, and the next two periods each contain 18 elements. The last two periods contain 32 elements. To make the table easier to read, some of these elements are placed at the bottom of the table. The table is organized so that elements with similar configurations of valence electrons are placed in the same column, or group. Atoms of elements in Group 1 (including hydrogen, lithium, and sodium) each have one valence electron. Atoms of elements in Group 17 (including fluorine, chlorine, and bromine) each have seven valence electrons. Valence electrons help determine the chemical properties of an element. This means that the elements in a group all have similar chemical properties. The Periodic Table can be used to predict many properties of elements. Metals are located on the left side and in the center of the table, while nonmetals are clustered on the right side. A staircase-like line divides the two groups. Elements called metalloids, which have some properties of metals and some properties of nonmetals, are located along this line.