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Matter Anything that has mass and takes up space.

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Presentation on theme: "Matter Anything that has mass and takes up space."— Presentation transcript:

1 Matter Anything that has mass and takes up space.
All matter can be measured Mass Volume Density

2 Hundreds of years ago, scientists found that certain types of matter couldn’t be broken down into any other simpler substances They called these special pure substances: elements

3 No matter how small you divide it, gold is only made of gold atoms.

4 So what is an atom? The smallest particle an element can be divided into and still maintain the properties of that element. Atoms are the building blocks of all matter.

5 Why learn about atoms? All matter is made of atoms, atoms are the basic building block of everything in the universe

6 What does an atom look like?
The model of the structure of the atom has changed as technology has improved and as more evidence has been gathered.

7 What are these made of?

8 (greek for indivisible)
HISTORY OF THE ATOM Democritus develops the idea of atoms 460 BC He pounded up materials in his pestle and mortar until he had reduced them to smaller and smaller particles which he called ATOMA (greek for indivisible)

9 First atomic models – roughly based on earth, air, water, and fire

10 What’s new?

11 HISTORY OF THE ATOM 1808 John Dalton Suggested that all matter was made up of tiny spheres that were able to bounce around with perfect elasticity and called them ATOMS

12 The new model of an atom- a tiny solid sphere

13 What’s new?

14 HISTORY OF THE ATOM Joseph John Thompson 1898 found that atoms could sometimes eject a far smaller negative particle which he called an ELECTRON

15 like plums surrounded by pudding.
Thompson develops the idea that an atom was made up of electrons scattered unevenly within an elastic sphere surrounded by a soup of positive charge to balance the electron's charge 1904 like plums surrounded by pudding. PLUM PUDDING MODEL

16 The new model of an atom- atoms contain smaller, negatively charged particles

17 What’s new?

18 1910 Ernest Rutherford English scientist who tested JJ Thompson’s model Rutherford’s new evidence allowed him to propose a more detailed model with a central nucleus. He suggested that the positive charge was all in a central nucleus. This held the electrons in place by electrical attraction

19 Rutherford’s experiment
His hypothesis: The results?

20 The new atomic model- a dense, positively charged nucleus in the center surrounded by electrons

21 What’s new?

22 Niels Bohr 1913 studied under Rutherford in Manchester, England Bohr refined Rutherford's idea by adding that the electrons were in orbits. Rather like planets orbiting the sun. With each orbit only able to contain a set number of electrons.

23 Bohr’s Atom electrons in orbits nucleus

24 The new atomic model- electrons are in orbits around the nucleus at different energy levels

25 What’s new?

26 1920’s Electron Cloud Model
Electrons surround the positively charged nucleus, but not in set orbits They are in different levels, or clouds There are set amounts of electrons found in each cloud

27 The new atomic model- set numbers of electrons are found in different cloud layers

28 Exit Slip Choose one of the atom models Draw a picture of it
Label it with the name of the model Give the date of when this model was first described Give a name to the chemist who described it Your name on the back

29 Atomic Model History http://www.youtube.com/watch?v=QbWKF9uDF7w

30 ATOMS AND ATOMIC STRUCTURE Atom Nucleus Proton Neutron Electron

31 WHAT IS AN ATOM? The smallest unit of an element.
Consists of a central nucleus surrounded by one or more electrons.

32 WHAT IS THE NUCLEUS? The central part of an atom.
Composed of protons and neutrons. Contains most of an atom's mass.

33 WHAT IS A PROTON? Positively charged particle.
Found within an atomic nucleus.

34 WHAT IS A NEUTRON? Uncharged particle. Found within an atomic nucleus.

35 WHAT IS AN ELECTRON? Negatively charged particle.
Located in shells that surround an atom's nucleus.

36 Summary Particle Charge Mass (amu) Location Proton positive 1 nucleus
Neutron neutral nucleus Electron negative < shells outside the nucleus

37 Atoms as Pictured on the Periodic Table
Atomic Number Symbol Name Atomic Mass protons electrons Atomic number equals the number of ____________ or ___________. protons neutrons Atomic mass equals the number of ______________ + ____________. (mass number)

38 How many protons? Same as the atomic number How many electrons? How many neutrons? Number of protons + ? = Atomic Mass

39 Atoms are neutral Since protons (positive charge) are equal to the numbers of electrons (negative charge), the overall charge of an atom is neutral

40 Video of particles http://www.youtube.com/watch?v=lP57gEWcisY Bill Nye

41 Let’s review The Atomic Number of an atom = number of ______________ in the nucleus. The Atomic Mass of an atom = number of _________ _________ in the nucleus. The number of Protons = Number of ____________. _____________ orbit the nucleus. Protons or electrons Protons neutrons electrons Electrons

42

43 Periodic Table blocks can sometimes contain even more information!

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