Key Terms: Nucleons Atomic Number Isotope Atomic Mass.

Slides:

Advertisements

Similar presentations

Atomic Number, Mass Number, Atomic Mass and Isotopes Mrs. Coyle Chemistry.

Advertisements

Chapter 5 Sections 2 and 3 Structure of an atom nucleus- center of an atom -discovered by Ernest Rutherford in 1911 proton (p+) -positively charged subatomic.

The Structure of the Atom The Building Block of Matter.

Isotopes. Subatomic Particles # protons = atomic number Carbon - atomic number 6; # of protons 6 # electrons (neutral atom) = # protons Carbon - # protons.

Atomic Structure Nucleus – contains protons and neutrons

OF PROTONS, NEUTRONS AND ELECTRONS IN AN ATOM

Atomic Mass & Number Isotopes The Periodic Table.

Essential Question: How do atoms of the same element differ?

Subatomic Particles and Isotopes. Subatomic Particles Protons- Positively Charged Protons- Positively Charged Located in the nucleus Located in the nucleus.

 Protons, neutrons, electrons too  Make up the atoms all around you!

Subatomic Particles. 1. Subatomic Particles ParticleSymbol (table O) ChargeMass (amu) Location Electrons e 0 e -1 0 β -1 Negative (-1) 1/1872 amu 0 amu.

Chemistry Ms. Pollock Introduction  Dalton’s atomic theory very good but not entirely correct  Atoms able to be broken into smaller particles.

Atomic Structure. Basic Parts of the atom- Subatomic Particles Proton Positive charge Found in the nucleus Dictate the identity of the atom Neutron No.

Atoms: The building blocks of Matter

Atomic Structure. Basic Parts of the atom- Subatomic Particles Proton Positive charge Found in the nucleus Dictate the identity of the atom Neutron No.

Objectives:  1. Name and describe the three subatomic particles in an atom.  2. Determine the number of protons, neutrons, and electrons in an atom or.

Components of the Atom Nucleus: Nuclear Forces:

Isotopes and Mass Number. Atomic Number The number of protons in each atom identifies it as an atom of a particular element Each atom has a unique number.

Subatomic Particles  Protons and electrons are the only particles that have a charge.  Protons and neutrons have essentially the same mass.  The mass.

Ch. 3 - Atomic Structure II. Masses of Atoms (p.75-80) Mass Number

Atomic Structure I. Subatomic Particles.

Distinguishing Among Atoms

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

How Atoms Differ.

Atomic Number, Mass Number, Atomic Mass and Isotopes

THE ATOM Counting. The Atom  Objectives Explain what isotopes are Define atomic number and mass number, and describe how they apply to isotopes Given.

Chapter 3 Atoms: The Building Blocks of Matter. The Atomic Theory  Law of conservation of mass  Mass is neither destroyed nor created  Law of definite.

Unit 2 Review - Section 1 Atomic Structure and Mass.

Counting Atoms 3.3. Counting Atoms Very difficult to count Atomic Number – # of p + of each atom of that element Whole numbers Elements arranged by atomic.

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

Proton, Neutron, Electron Counting Protons (p + ) are positively charged and located in the nucleus The number of protons in each atom can be found on.

Ch. 3 - Atomic Structure II. Masses of Atoms (p.75-80)  Mass Number  Isotopes  Relative Atomic Mass  Average Atomic Mass.

Section 4.3 How atoms differ. Atomic Number Represents three things in a neutral atom: 1. What element it is 2. The number of protons in each atom 3.

Average Atomic Mass. Relative Atomic Masses  Masses of atoms (in grams) are very small, so for convenience we use relative masses.  Carbon-12 is our.

I. Subatomic Particles (p ). ParticleSymbolLocationChargeRelative Mass (amu) Actual Mass (g) electron proton neutron e-e- p+p+ n0n0 Electron.

D. Subatomic Particle & the Nuclear Atom 1.Nucleus contains positively charged protons and neutral neutrons VERY dense! If a nucleus were the size of the.

Calculating Particles in a atom

Unit 3: Atomic Structure. A. Subatomic Particles Most of the atom’s mass (Mass Number) NUCLEUS ELECTRON CLOUD PROTONS NEUTRONS ELECTRONS POSITIVE CHARGE.

Isotopes. Let’s Review ProtonsNeutronsElectrons Charge +1 0 Mass 1 amu 0 Location nucleus Electron cloud.

Atom – basic unit of matter 3 subatomic particles: protons, electrons, neutrons Atom is mostly empty space Atoms have small dense positive core (nucleus)

Atomic Structure. I. Atoms The atom is the basic unit of matter.

Atomic Structure What are atoms made of? How are atoms put together? What are Elements? Isotopes?

Unit 3: The Atom. Atoms All matter is made of very tiny particles All matter is made of very tiny particles These particles have the same properties as.

Notes on Isotopes Remember Protons are (+) and Electrons are (-). Neutrons were the last subatomic particles to be discovered because they have no electrical.

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

Notes on Isotopes Remember Protons are (+) and Electrons are (-). Neutrons were the last subatomic particles to be discovered because they have no electrical.

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

Parts of the Atom … from Discovery to Reality. NUCLEUS PROTONS ✚ Positively charged particles Mass = 1 amu NEUTRONS No charge or neutral Mass = 1 amu.

 Atom – the smallest particle of an element that retains the properties of that element.  When we say “small,” we mean “SMALL!”  A typical copper penny.

Atomic Structure Review Which of the following is NOT true about electrons? a) They have a negative charge b) They are the heaviest subatomic particle.

UNIT 3: DAY 1 AND DAY 3 ATOMIC STRUCTURE. ATOM, ELEMENTS, AND COMPOUNDS Atoms are the smallest unit of matter In classification, all atoms are elements.

Isotopes and abundance. The relative atomic mass scale is now based on an isotope of carbon, carbon-12, which is given the value of amu.

Atomic Structure Notes Subatomic Particles Subatomic Particles Atomic Number, Atomic Mass & Mass Number Atomic Number, Atomic Mass & Mass Number Symbols.

The Structure of Atoms Section 4.2. You want to be able to … describe the general structure of the atom, and explain how the properties of the first 20.

 Atoms  Elements are made of particles called atoms  Atoms are the smallest pieces of matter that contain all the properties of a specific element.

Atomic Structure.

Atomic Structure Subatomic Particles C. Johannesson.

Subatomic Particles Masses of Atoms Mass Number Isotopes Ions

Atomic Particles Particle Charge Mass # Location Electron -1

Section 3 Counting Atoms

Ch. 3 - Atomic Structure II. Masses of Atoms (p.75-80) Mass Number

The Atom Unit 2 Topic 1.

Atomic Structure Protons- positively charged, found in nucleus

Atomic Structure Nucleons Atomic Number

Protons & Neutrons.

Ch. 4 - Atomic Structure II. Masses of Atoms Mass Number Isotopes

The Atom Ch 3.1.

Presentation transcript:

Key Terms: Nucleons Atomic Number Isotope Atomic Mass

 Particles in the nucleus of atoms ◦ Protons ◦ Neutrons  These particles are “bound” together to form the dense positively charged nucleus that was discovered by Rutherford’s experiments

 Equal the number of protons in the nucleus on an atom  Seen on the periodic table as a whole number  The number or protons determines the identity of the element ◦ 6 protons is a carbon atom  Neutral atom- ◦ Number of protons (positive) = number of electrons (negative)

 Atoms of an element that have different numbers of neutrons  For carbon there are 2 predominate isotopes: ◦ 12 C at 98.9% abundance ◦ 13 C at 1.1% abundance  The above notation in known as nuclear symbol notation  There is also hyphen notation ◦ Carbon-12 and Carbon-13

Mass spectrometry is a method for seeing isotopes and their respective ratios (CuI) 3

 Hydrogen-1 ◦ 1 proton and 0 neutrons  Hydrogen-2 ◦ 1 proton and 1 neutron  Hydrogen-3 ◦ 1 proton and 2 neutrons  What is the nuclear notation for these? ◦1H◦1H ◦2H◦2H ◦3H◦3H

 Write the following elements in the opposite notation given. 1.Copper-63  63 Cu 2. 7 Li  Lithium-7 3.Silver-108  108 Ag Ne  Neon-22

 Total number of protons and neutrons in an atom  The mass number is always a whole number  Looking at Carbon-12, how many protons and neutrons? ◦ 6 protons and 6 neutrons  Number of neutrons = mass number - protons  Electrons are ignored in mass number calculations because they weigh 1/2000 th of a proton

 How many protons and neutrons are in 63 Cu? ◦ Atomic number = 29  number of protons ◦ 63 mass number – 29 protons = 34 neutrons  How many protons and neutrons are in 39 K? ◦ Atomic number = 19  number of protons ◦ 39 mass number – 19 protons = 20 neutrons

 Average of the masses of all element’s isotopes  How do we arrive at g/mol if protons and neutrons each weigh 1 amu? ◦ The average of all of the abundances of isotopes can be used to calculate the atomic mass of an element

 Using isotopes we can solve for the Atomic Mass of an element using the following equation:  (mass of isotope A)(Percent abundance of A) + (mass of isotope B)(Percent Abundance of B) +…. = Molar Mass

 For carbon there are 2 predominate isotopes: ◦ 12 C at 98.9% abundance ◦ 13 C at 1.1% abundance Molar Mass = 12* *0.011 Molar Mass = Molar Mass = g/mol

 Isotopes of potassium are: ◦ 39 K at 93.26% abundance ◦ 40 K at 0.012% abundance ◦ 41 K at 6.73% abundance Molar Mass = 39* * * Molar Mass = Molar Mass = 39.1 g/mol

 Isotopes of Silver are: ◦ 107 Ag at % abundance ◦ 109 Ag at % abundance Molar Mass = 107* * Molar Mass = Molar Mass =

ParticleChargeMassLocation Proton+11 amuNucleus NeutronNeutral1 amuNucleus Electron0Electron cloud

 Number of protons? ◦ 26  Number of electrons? ◦ 26  Number of neutrons? ◦ 30

 Number of protons? ◦8◦8  Number of electrons? ◦8◦8  Number of neutrons ◦8◦8