Chapter 12.1 Learning Goals  Apply an understanding of electric charge to describe the structure of atoms.  Identify and describe particles which comprise.

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Presentation transcript:

Chapter 12.1 Learning Goals  Apply an understanding of electric charge to describe the structure of atoms.  Identify and describe particles which comprise atoms.  Compare and contrast forces inside atoms.

Investigation 12A  Key Question: What is inside an atom? Atomic Structure

12.1 Structure of the Atom  In order to understand atoms, we need to understand the idea of electric charge.  We know of two different kinds of electric charge and we call them positive and negative.

12.1 Electric charge in matter  Scientists use the letter e to represent the elementary charge.  At the size of atoms, electric charge always comes in units of +” or “–”.  Electric charge appears only in whole units of the elementary charge.

12.1 Inside an atom  The mass of the nucleus determines the mass of an atom because protons and neutrons are much larger and more massive than electrons.  In fact, a proton is 1,836 times heavier than an electron.

12.1 Force inside atoms  Electrons are bound to the nucleus by the attractive force between electrons (-) and protons (+).

12.1 Force inside atoms  What holds the nucleus together?  There is another force that is even stronger than the electric force.  We call it the strong nuclear force.

12.1 How atoms of various elements are different  The atoms of different elements contain different numbers of protons in the nucleus.  Because the number of protons is so important, it is called the atomic number.

12.1 Atomic number and protons  Each element has a unique atomic number.  Atoms of the same element always have the same number of protons in the nucleus.

12.1 Ions  Complete atoms have a net zero charge.  Ions are atoms that have a different number of protons than electrons and so they have a positive or negative charge.

12.1 How atoms of various elements are different  Isotopes are atoms of the same element that have different numbers of neutrons.  The mass number of an isotope tells you the number of protons plus the number of neutrons. How are these carbon isotopes different?

Solving Problems  How many neutrons are present in an aluminum atom that has an atomic number of 13 and a mass number of 27?

 Looking for:  …number of neutrons in aluminum-27  Given  … atomic no. = 13; mass no. = 27  Relationships:  Periodic table says atomic no. = proton no.  protons + neutrons = mass no.  Solution  neutrons = mass no. – protons  neutrons = 27 – 13 = 14 Solving Problems