Matter and Atomic Structure Chap. 3 What are elements? How atoms combine States of matter States of matter

What makes a gold atom different from a silver atom?

What are elements? – 3.1 Objectives Describe the particles within atoms and the structure of atoms Relate the energy levels of atoms to the chemical properties of elements Define the concept of isotopes

I.Element

Element Substance that cannot be broken down into simpler substance by physical or chemical means.

I.Element A.Element names Carbon C

I.Element A.Element names B.Element symbols Carbon C

I.Element A.Element names B.Element symbols C.Elements are made of atoms

II. Atoms

Atom Smallest particle of an element.

II. Atoms A.Composed of 3 particles

II. Atoms A.Composed of 3 particles 1. Protons

II. Atoms A.Composed of 3 particles 1. Protons 2. Neutrons

II. Atoms A.Composed of 3 particles 1. Protons 2. Neutrons nucleus

II. Atoms A.Composed of 3 particles 1. Protons 2. Neutrons 3. Electrons

II. Atoms A.Composed of 3 particles B.Atomic number

proton neutron Atomic number Number of protons.

proton neutron Atomic number Number of protons. 5

II. Atoms A.Composed of 3 particles B.Atomic number C.Mass number

proton neutron Mass number Sum of the number of protons and neutrons

proton neutron Mass number Sum of the number of protons and neutrons 11

II. Atoms D.Electrons in Energy Levels

Electron Energy Levels Energy levelElectron Capacity First 2 Second8 Third18 Fourth32

Model of Oxygen

Self Check – Ex. 1 Draw a model of the lithium-7 atom. Include protons, neutrons, and electrons.

Self Check – Ex. 2 Draw a model of the chlorine-35 atom. Include protons, neutrons, and electrons.

1. Core electrons II. Atoms D.Electrons in Energy Levels

1. Core electrons 2. Valence electrons II. Atoms D.Electrons in Energy Levels

Valence electron Outermost electron found in a shell.

III. Isotopes

Isotopes Atoms with the same number of protons, but different numbers of neutrons.

III. Isotopes A.Isotopes have different masses

III. Isotopes A.Isotopes have different masses B.Nature contains a variety of isotopes

III. Isotopes A.Isotopes have different masses B.Nature contains a variety of isotopes C.Isotopes used to find atomic mass of element

Atomic mass The average of the masses of each isotope present for a give element.

III. Isotopes D.Radioactivity

Radioactivity The spontaneous decay of an atom’s nucleus into a new nucleus.

IV. Abundance A.In Universe

Abundance in Universe

IV. Abundance A.In Universe B.In Earth’s crust

Abundance in Earth’s Crust

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How atoms combine – 3.2 Objectives Describe the chemical bonds that unit atoms to form compounds Relate the nature of chemical bonds that hold compounds together to the physical structures of compounds Distinguish between different types of mixtures and solutions

I.Compounds

Compound More than one element chemically combined.

I.Compounds A.Covalent compounds share electrons

I.Compounds A.Covalent compounds share electrons 1. Sharing electrons helps atoms get full electron set

I.Compounds A.Covalent compounds share electrons 1. Sharing electrons helps atoms get full electron set 2. Sharing may not be equal: this makes polar molecules

I.Compounds B.Ionic compounds transfer electrons

I.Compounds B.Ionic compounds transfer electrons 1. When an atom gains an electron it becomes _______

I.Compounds B.Ionic compounds transfer electrons 1. When an atom gains an electron it becomes _______ 2. When an atoms loses an electron it becomes _______

Ion An atom that has gained or lost an electron.

I.Compounds B.Ionic compounds transfer electrons 1. When an atom gains an electron it becomes _______ 2. When an atoms loses an electron it becomes _______ 3. Opposites _______

I.Compounds C.Metallic bonds have a ‘sea of electrons'

II. Reactions

A.Bonds are broken and reformed

II. Reactions A.Bonds are broken and reformed B.New substances are formed

II. Reactions A.Bonds are broken and reformed B.New substances are formed C.Energy is exchanged

III. Mixtures

A.Most mixtures are heterogeneous

Heterogeneous A mixture with visibly different parts.

III. Mixtures A.Most mixtures are heterogeneous B.Mixtures that are homogeneous are called solutions

Homogeneous A mixture with the same makeup throughout.

IV. Acids & Bases

A.An acid makes H + ions

IV. Acids & Bases A.An acid makes H + ions B.A base produces OH - ions

IV. Acids & Bases A.An acid makes H + ions B.A base produces OH - ions C.The pH scale tells how acidic/basic something is

The pH Scale acidic basicneutral

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States of Matter – 3.3Objectives Describe the states of matter on Earth Explain the reasons that matter exists in these states Relate the role of thermal energy to changes of state in matter

I. The Four Phases of Matter

A.Solid

I. The Four Phases of Matter A.Solid 1. solids with regular structure are described as crystalline.

I. The Four Phases of Matter A.Solid 1. solids with regular structure are described as crystalline. 2. in some solids there is no organized pattern. These are amorphous.

I. The Four Phases of Matter A.Solid B.Liquid

I. The Four Phases of Matter A.Solid B.Liquid C.Gas

I. The Four Phases of Matter A.Solid B.Liquid C.Gas 1. gases have undergone vaporization or sublimation

Evaporation Changing from liquid to vapor

Sublimation Changing from solid to vapor

I. The Four Phases of Matter A.Solid B.Liquid C.Gas 1. gases have undergone vaporization or sublimation 2. gas particles are separated by large distances

I. The Four Phases of Matter A.Solid B.Liquid C.Gas D.Plasma

Plasma Hot, highly ionized, electrically conducting gas.

II. Changes in State

A.When a liquid changes to a gas, heat is _______.

II. Changes in State A.When a liquid changes to a gas, heat is _______. B. When a gas changes to a liquid, heat is _______.

The End