1. Earth Chemistry Section 1 Section 1: Matter Preview Objectives Comparing Physical and Chemical Properties Properties of Matter Atomic Structure Parts of the Atom Atomic Number Periodic Table Overview Atomic Mass Valence Electrons and Periodic Properties

2. Earth Chemistry Section 1 Objectives Compare chemical properties and physical properties of matter. Describe the basic structure of an atom. Compare atomic umber, mass number, and atomic mass. Define isotope. Describe the arrangement of elements in the periodic table.

3. Earth Chemistry Section 1 Properties of Matter matter * Every object in the universe is made up of particles of matter. The amount of matter in any object is the mass of that object. All matter has two types of distinguishing properties-*.

4. Earth Chemistry Section 1 Properties of Matter, continued Physical properties are characteristics that can be observed without changing the composition of the substance. Physical properties include density, color, hardness, freezing point, boiling point, and the ability to conduct an electric current. Chemical properties are characteristics that describe how a substance reacts with other substance to produce different substances.

5. Earth Chemistry Section 1 Properties of Matter, continued Elements element a substance that cannot be separated or broken down into simpler substances by chemical means; Each element has a characteristic set of physical and chemical properties that identify it. Every known element is represented by a symbol of one or two letters.

6. Earth Chemistry Section 1 Properties of Matter, continued Atoms Elements are made of atoms. atom * A single atom is so small that its size is difficult to imagine.

7. Earth Chemistry Section 1 Atomic Structure Even though atoms are very tiny, they are made up of smaller parts called subatomic particles. There are three types of subatomic particles—protons, electrons, and neutrons. proton * electron * neutron *

8. Earth Chemistry Section 1 Atomic Structure, continued The Nucleus The protons and neutrons of an atom form the nucleus. The positively charged nucleus makes up most of an atom’s mass but very little of its volume. The volume of an atom is mostly empty space. The Electron Cloud The electrons of an atom move in a certain region of space called an electron cloud that surrounds the nucleus. The negatively charged electrons are attracted to the positively charged nucleus. This attraction holds electrons in the atom.

9. Earth Chemistry Section 1 Parts of the Atom

10. Earth Chemistry Section 1 Atomic Number The number of protons in the nucleus of an atom is called the atomic number. All atoms of any given element have the same atomic number. An element’s atomic number sets the atoms of that element apart from the atoms of all other elements. Elements on the periodic table are ordered according to their atomic numbers. Elements in the same column on the periodic table have similar arrangements of electrons in their atoms, and therefore have similar chemical properties.

11. Earth Chemistry Section 1 Atomic Number, continued The diagram below shows the atomic numbers and mass numbers of three elements.

12. Earth Chemistry Section 1 Atomic Number, continued The diagram below shows the periodic table.

13. Earth Chemistry Section 1 Periodic Table Overview

14. Earth Chemistry Section 1 Atomic Mass The sum of the number of protons and neutrons in an atom is the mass number. The mass of a subatomic particle is too small to be expressed easily in grams, so a special unit called the atomic mass unit (amu) is used. Protons and neutrons each have an atomic mass close to 1 amu. Electrons have much less mass than protons or neutrons do. The mass of 1 proton is equal to the combined mass of about 1,840 electrons.

15. Earth Chemistry Section 1 Atomic Mass, continued Isotopes Although all atoms of a given element contain the same number of protons, the number of neutrons may differ. isotope * Because of their different number of neutrons and their different masses, different isotopes of the same element have slightly different properties.

16. Earth Chemistry Section 1 Atomic Mass, continued Average Atomic Mass Because isotopes of an element have different masses, the periodic table uses an average atomic mass of each element. The average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of an element.

17. Earth Chemistry Section 1 Valence Electrons and Periodic Properties Based on similarities in their chemical properties, elements on the periodic table are arranged in columns, which are called groups. An atom’s chemical properties are largely determined by the number of the outermost electrons in an atom’s electron cloud. These electrons are called valence electrons. The elements that form each group commonly have the same number of valence electrons.

18. Earth Chemistry Section 1 Valence Electrons and Periodic Properties, continued When an atom has 8 valence electrons, it is considered stable, or chemically unreactive. Unreactive atoms do not easily lose or gain electrons. Elements whose atoms have only one, two, or three valence electrons tend to lose electrons easily. These elements have metallic properties and are generally classified as metals. Elements whose atoms have from four to seven valence electrons are more likely to gain electrons. Many of these elements are classified as nonmetals.