The Atom Three Basic Particles. Proton Nucleus of atom Positive charge # of protons (p + ) = atomic number Contain much of the mass of the atom.

Slides:

Advertisements

Similar presentations

Reviewing Subatomic Particles

Advertisements

Bellringer Write down 5 things you know about atoms.

Atomic Structure Section The Nucleus Nucleus- contains most of the mass of an atom – Protons & Neutrons contains most of an atom’s mass – Electrons-

Atomic Structure.

Atomic Mass & Number Isotopes The Periodic Table.

The Periodic Table. Define the following terms. 1. proton 2. neutron 3. electron 4. nucleus.

Seconds Left: A stable carbon atom has the following parts: – 6 protons – 6 neutrons.

Atoms Atomic Mass/Number Ions/Charges of Molecules Isotopes/Perc ent Abundance

Explaining the Periodic Table (6.7) If elements are the building blocks of all other matter, what are they made of? There are three particles that make.

 The atoms of all elements are made up of a central nucleus with orbiting electrons. ◦ A nucleus is made up of positively charged PROTONS and neutral.

Mass Number Atomic Number equals the # of... NUCLEUS ELECTRONS PROTONS NEUTRONS NEGATIVE CHARGE POSITIVE CHARGE NEUTRAL CHARGE ATOM.

THE STRUCTURE OF ATOMS Pg. 43. Daily science- pg. 40  Who discovered the neutron? Electron? Nucleus?  What did Democritus theorize?  Name two differences.

Atomic Structure.

Building Blocks 1c Int

Matter & The Atom. Matter The term matter describes all of the physical substances around us Matter is anything that has mass and takes up space The Universe.

Atomic Structure lecture 4.1. Atomic structure Small, dense nucleus Protons: (+) charge Neutrons : (0) no charge Electrons: (-) charge # Protons = # electrons.

Atomic Structure Chm Matter MixturesPure Substances.

Atom Notes Notebook /22/02 What is in an atom? The Three Primary Subatomic Particles... n Protons n Neutrons n Electrons.

Chapter 2~The Chemistry of Life

Vocabulary ATOM-the smallest unit that maintains the characteristics of an element – Nucleus- The center of the atom, contains protons and neutrons –

Ions, Complete Chemical Symbols and Isotopes. Every element is made up of very small particles called atoms. Atoms of different elements have a different.

Atoms. What are atoms? All matter is made of atoms Atoms are the smallest part of an element (1 million times smaller than the width of 1 piece of hair)

The Atom the smallest unit of an element protons and neutrons in nucleus surrounded by one or > shells of electrons neutral atoms: # protons = # electrons.

Unit 2 Review - Section 1 Atomic Structure and Mass.

“CHEMISTRY OF LIFE” Chapter 6. ELEMENTS: A SUBSTANCE THAT CAN NOT BE BROKEN DOWN INTO A SIMPlER SUBSTANCE. ELEMENTS CONSIST OF ONE TYPE OF ATOM. These.

Determining the NUMBER of Protons Electrons and Neutrons in Atoms, Ions, and Isotopes.

Rutherford Experiment & Isotopes Mr. Rana 9/21/12.

Atomic Structure Revision Atoms and the periodic table 1. What is the charge on a neutron? 2.What is the mass of an electron? 3.What is the positive particle.

Atomic Structure nucleusproton (+) Neutron (o) Electron (-)

Isotopes and Ions.

Atomic Structure SOL 6.4.

What Makes Up a Atom?. Atoms are the smallest unit of matter. Atoms are the smallest unit of matter. Atoms CANNOT be divided! Atoms CANNOT be divided!

ParticleSymbolRelative Charge Relative Mass (proton = 1) Actual Mass (g) Electrone-e- 1-1/ X Protonp+p x Neutronn0n x10.

Atoms Atom- the smallest part of an element Atoms of one element are different from another element. contains protons, electrons, and neutrons Atomic Mass.

Matter & The Atom. Matter The term matter describes all of the physical substances around us Matter is anything that has mass and takes up space The Universe.

Atom Notes Pre-test (answer at the top of your paper) 1. How many protons, neutrons, & electrons does Magnesium have? 2. What is the Atomic Number of.

Isotopes and Ions. Isotopes Atoms of the same element that have different masses Have the same number of protons and electrons but different numbers of.

Atoms and the Periodic table v=pO0X6fVre1I&feature=related v=pO0X6fVre1I&feature=related

What part of an atom is the arrow pointing to? A. proton B. electron C. neutron D. shell E. nucleus.

Atomic Mass. Each element found on the periodic table of elements is given an atomic mass The atomic mass tells you the average mass of the atoms of an.

Parts of the Atom: Properties  Protons: –Positive charge –Located in nucleus –Mass = 1 amu (Atomic Mass Unit)  Neutrons –No charge (neutral) –Inside.

Atomic Number The number of protons in an atom Also, the number of electrons in a neutral atom.

Atoms. Structure of Atoms  Atoms are made up of subatomic particles:

There are three states of matter: gas, solid and liquid All matter is made of atoms An element is made up of one type of atom A molecule is a combination.

1Chemistry Chapter 4: How Atoms Differ: Atomic number = # p + AND e - (assume neutral atom for charge). Atomic number = # p + AND e - (assume neutral atom.

EQ: What are the two types of chemical bonds and what makes each one unique?

The Structure of an Atom

ELECTRONS. Review Electrons were discovered by ______________ Electrons have a ___________ charge Electrons are located…. Outside of the nucleus in an.

Ion a particle that is electrically charged (positive or negative); an atom or molecule or group that has lost or gained one or more electrons Ions DO.

Isotopes Chapter 4, Section 3 Pg Review of Atoms Atoms are made of protons, neutrons, and electrons. – Protons are +, electrons are –, and.

{ Atom and Isotope Review Physical Science. An atom has 6 protons, 8 neutrons, and 6 electrons. What is the atomic mass?

2. What are isotopes? Use two particles from the table above to illustrate your answer. (3 marks) 17 O & 18 O (1) Same Atomic mass / number of protons.

Subatomic Particles. Using the Periodic Table N Atomic Number Mass Number Symbol.

1 The Atom Atomic Number and Mass Number Isotopes.

The Atomic Theory The smallest particle of an element that can enter into chemical change. 2. Building block of all matter. 3. Consists of a central nucleus.

ELEMENTS, IONS AND ISOTOPES

Isotopes and Ions Do Now – Explain how atoms of different elements differ from one another. Give a specific example.

Atomic Structure Nat

Atomic Number Atomic Mass

Atomic Structure Most of the mass of an atom is concentrated in an extremely small, dense, and positively charges core called the nucleus The nucleus contains.

Atomic Structure.

Structure of an Atom.

Isotopes & Ions.

What is the basic structure of an Atom?

Atomic Structure Nucleus Protons Neutrons Electrons.

Presentation transcript:

The Atom Three Basic Particles

Proton Nucleus of atom Positive charge # of protons (p + ) = atomic number Contain much of the mass of the atom

Neutron Nucleus of atom Nucleus of atom No charge (neutral) No charge (neutral) Mass # = # of protons + # of neutrons (n o ) Mass # = # of protons + # of neutrons (n o ) Help to keep the nucleus stable Help to keep the nucleus stable The number of neutrons determines the isotope of the element The number of neutrons determines the isotope of the element Contain much of the mass of the atom Contain much of the mass of the atom

Electron Orbiting outside of the nucleus Orbiting outside of the nucleus Electrons (e - ) can be added or removed from atoms to create ions and form chemical bonds Electrons (e - ) can be added or removed from atoms to create ions and form chemical bonds Negative charge Negative charge # of e - = # of p + (in a neutral atom) # of e - = # of p + (in a neutral atom) Very negligible mass Very negligible mass protons and neutrons are roughly the same mass as each other and are about 1800 times heavier than electrons protons and neutrons are roughly the same mass as each other and are about 1800 times heavier than electrons

How small are atoms? TRY THIS !!! If the radius of a sodium atom is 186 picometers, then calculate the # of sodium atoms that would line up side by side on a line that is 5.00 cm long … (Hint: 1 pm = cm)

Ready for the answer?

WOW!!!

How did you get that? 1)Radius x 2 = Diameter 186 pm x 2 = 372 pm 2)5.00 cm=5.00 cm= 372 pm cm sodium atoms!!

More about Isotopes Isotopes  atoms of the same element that have different masses are called isotopes  Different masses are caused by different numbers of neutrons  Example: Uranium–235 and Uranium–238 Both are Uranium, so both have 92 protons, but U-235 has 143 neutrons and U-238 has 146 neutrons (so the U-238 isotope is a little bit heavier)

Isotope Symbols U-238 U-238 Mass Number (# of protons + # of neutrons) U Mass Number (# of protons + # of neutrons) Atomic Number (# of protons) Al 3+ Charge (lost 2 electrons) to make a positive ion 26 13