Warm up 9/14/15 Draw a detailed picture of an atom. (Think about what you may have learned in middle school. What makes up an atom?)Draw a detailed picture.

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Presentation transcript:

Warm up 9/14/15 Draw a detailed picture of an atom. (Think about what you may have learned in middle school. What makes up an atom?)Draw a detailed picture of an atom. (Think about what you may have learned in middle school. What makes up an atom?)

Atoms: The Building Blocks of Matter Chapter 3

Atoms, Compounds & Molecules Atoms: the smallest particle of an element that retains the chemical properties of that element.Atoms: the smallest particle of an element that retains the chemical properties of that element. Compound: a substance that consists of two or more different types of elements.Compound: a substance that consists of two or more different types of elements. Molecule: a substance that consists of two or more atoms.Molecule: a substance that consists of two or more atoms. Ion: An atom or molecule with a net electric charge due to the loss or gain of electrons.Ion: An atom or molecule with a net electric charge due to the loss or gain of electrons.

Dalton: Basic Atomic Theory 1.All matter is made of atoms.

2. Atoms of one element differ in properties (size, mass etc…) from atoms of another element.

3. Atoms of different elements combine in simple, whole-number ratios to form molecules.

4. In chemical reactions atoms can combine, separate and rearrange, but not destroyed.

Structure of the Atom Atoms consist of two regions:Atoms consist of two regions: 1. Nucleus : Which is a very small region located in the center of an atom which contain positively (+) charged particles called protons and one or more (=) neutral particles called neutrons. 2. Electron cloud: A region very large compared to the nucleus which contains very small negatively (-) charged particles called electrons.

Structure of the Atom Neutrons, protons and electrons are called the subatomic particles.Neutrons, protons and electrons are called the subatomic particles. Electrons are much smaller in size and mass than neutrons and protons.Electrons are much smaller in size and mass than neutrons and protons.

Discovery of the Electron Cathode-ray tube experiments performed by JJ Thompson provided evidence that all atoms contained negatively charged particles.Cathode-ray tube experiments performed by JJ Thompson provided evidence that all atoms contained negatively charged particles.

Questions raised by the discovery of the electron If it is true that all atoms have these super tiny negatively charged particles two main questions arise:If it is true that all atoms have these super tiny negatively charged particles two main questions arise: 1.Because atoms are electrically neutral, they must contain a positive charge to balance out negative electrons 2.Because electrons have so much less mass than atoms, atoms must contain other particles that account for most of their mass.

Discovery of the Atomic Nucleus Rutherford discovered that all atoms have a very small, dense and positively charged nucleus by performing what we call the “gold foil experiment.”Rutherford discovered that all atoms have a very small, dense and positively charged nucleus by performing what we call the “gold foil experiment.”

Rutherford’s Conclusions Most of the mass and all of the positive charge of the atom is in a very dense nucleus.Most of the mass and all of the positive charge of the atom is in a very dense nucleus. However the nucleus only takes up a very small space in an atom.However the nucleus only takes up a very small space in an atom. Atoms are mostly empty space.Atoms are mostly empty space. EXAMPLE: If the nucleus of an atom was the size of a marble, the size of the atom would be equal to a football field. EXAMPLE: If the nucleus of an atom was the size of a marble, the size of the atom would be equal to a football field.

Atomic Number Atomic Number: (Z) tells you how many protons are in each atom of an element. The atomic # identifies the element.Atomic Number: (Z) tells you how many protons are in each atom of an element. The atomic # identifies the element. Chemical (Atomic) Symbol: Is the letter abbreviation for an element.Chemical (Atomic) Symbol: Is the letter abbreviation for an element. Atomic Number = 6 Chemical Symbol

Examples! How many protons are in each of the following:How many protons are in each of the following:

From yesterday… Which 2 subatomic particles did we say are the biggest/ make up most of an atom’s mass?Which 2 subatomic particles did we say are the biggest/ make up most of an atom’s mass?

Mass Number Mass Number: (A) is the total number of protons and neutrons that make up the nucleus of an atom.Mass Number: (A) is the total number of protons and neutrons that make up the nucleus of an atom. Mass Number (A) – Atomic Number (Z) = Number of Neutrons Mass Number (A) – Atomic Number (Z) = Number of Neutrons Mass Number can be written two ways:

Be Able to Interpret

With your group… Can the atomic number ever be bigger than the mass number? Why or why not?Can the atomic number ever be bigger than the mass number? Why or why not?

Example! How many protons, neutrons, and electrons are in Carbon 14?

Warm Up 9/21/15 Why are isotopes important?Why are isotopes important?

isotopes Isotopes: are atoms of the same element that have different masses.Isotopes: are atoms of the same element that have different masses. Isotopes of a particular element all have the same number of protons and electrons, but different numbers of neutrons.Isotopes of a particular element all have the same number of protons and electrons, but different numbers of neutrons.

Reading Isotopes

Average Atomic Mass Although isotopes have different masses, they do not differ significantly in their chemical behavior.Although isotopes have different masses, they do not differ significantly in their chemical behavior. Average atomic mass: the weighted average of the atomic masses of the naturally occurring isotopes of an element.Average atomic mass: the weighted average of the atomic masses of the naturally occurring isotopes of an element. Basically two things matter: the mass and relative abundance of an elements isotopes.Basically two things matter: the mass and relative abundance of an elements isotopes.

Nitrogen A sample of nitrogen is tested and has a two isotopes of nitrogen % of atoms are N- 14 and 0.36% atoms are N-15. What is the average atomic mass?A sample of nitrogen is tested and has a two isotopes of nitrogen % of atoms are N- 14 and 0.36% atoms are N-15. What is the average atomic mass?

ions An ion is an atom or a molecule in which the total number of electrons IS NOT EQUAL to the number of protons. This gives the atom or molecule a net positive or negative ELECTRICAL CHARGE.An ion is an atom or a molecule in which the total number of electrons IS NOT EQUAL to the number of protons. This gives the atom or molecule a net positive or negative ELECTRICAL CHARGE.

CATION If a neutral atom loses one or more electrons, it has a net POSITIVE charge, and is called a CATION.If a neutral atom loses one or more electrons, it has a net POSITIVE charge, and is called a CATION.

anion If an atom gains electrons, it has a net NEGATIVE charge and is called an ANION.If an atom gains electrons, it has a net NEGATIVE charge and is called an ANION.

Who Cares? A lithium-ion battery is a rechargeable battery used in lots of cell phones and cameras. Lithium ions move from the negative electrode to the positive electrode during discharge and back when charging.