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Atomic Structure. Define the atom Structure of the Nuclear Atom Distinguish between atoms. In groups of 7 you will research the following scientists’ ideas and contributions to the atomic model.

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atomic structure

AtomicStructure

Define the atom

Structure of the Nuclear Atom

Distinguish between atoms

early models of the atom

In groups of 7 you will research the following scientists’ ideas and contributions to the atomic model.

  • 1. John Dalton, 2. Democritus, 3. J.J Thomson, 4. Ernest Rutherford, 5. Robert Millikan,

6. Eugen Goldstein, 7. James Chadwick

  • You will present your findings to the class
Early Models of the Atom
what are the 3 kinds of subatomic particles

? Charge

? Location

? Symbol

protons

What are the 3 kinds of subatomic particles?

neutrons

electrons

what makes one element differ from another

23

V

50.941

Atomic

number

symbol

  • The Number of protons (atomic number)
  • Atoms are electrically neutral; therefore the number of protons (+) must equal the number of electrons (-)

Average

Atomic mass

Try these!

What makes one element differ from another?

6

how do you find the of neutrons

Find the difference between the mass number and atomic number

Atomic number

?

# of protons

14

Si

28.086

# of electrons

Average atomic mass

?

Round this for mass number

How do you find the # of neutrons?

Mass number =

Atomic number =

Number of neutrons=

shorthand notation

1.Write the symbol, place the atomic number as the subscript and the mass number as the superscript to the left of the symbol.

14

Si

28.086

Si

28

14

  • Also can be written with the name of the symbol
  • and the mass number
Shorthand notation

Silicon-28

practice

A.

  • How many neutrons are in each atom?

16

8

O

32

16

S

108

47

Ag

practice

p+ =

e- =

n0=

p+ =

e- =

no =

p+ =

e- =

no =

slide8

Tellurium

Remember!!Atomic # = protons = electronsMass # = Protons + NeutronsNeutrons = Mass # - ProtonsProtons = Mass # - Neutrons

isotopes

Atoms that have the same number of protons, but different numbers of neutrons, therefore having different mass numbers

  • Isotopes are chemically alike due to the # of protons and electrons
  • There are 3 known isotopes of hydrogen.
  • Each isotope has one proton
  • Most common = hydrogen-1 or H
  • 2nd isotope has one neutron (mass # of 2) = _____________or hydrogen-2 or H
  • 3rd isotope has 2 neutrons (mass # of 3) =
  • ___________or hydrogen-3 or H

1

1

2

1

Isotopes

3

1

practice1

Three isotopes of oxygen are oxygen-16, oxygen-17, oxygen-18. Write the symbol for each, including the atomic number and mass number.

  • Three isotopes of chromium are chromium-50, chromium-52, and chromium-53. How many neutrons are in each isotope, given that chromium has an atomic number of 24?

16

8

O

17

8

O

18

8

O

Practice

Chromium-50 = ____ neutrons

Chromium-52 = ____neutrons

Chromium-53 = ____ neutrons

extra credit

Research common isotopes (radioistopes)

  • Create a display over commonly used isotopes.
  • Include the isotope and its use
  • Also may include pictures, etc.
Extra Credit
slide12

Atomic Mass

  • Atomic mass unit- (amu)-
  • Atomic mass=

Calculating the atomic mass

Multiply the mass of each isotope by the natural abundance, expressed as a decimal, and then add the products

slide13

Element X has 2 natural isotopes. The isotope with a mass of 10.012 amu (10X) has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu (11X) has a relative abundance of 80.09%. Calculate the atomic mass of this element

knowns

unknowns

Practice

Calculate

For 10X: 10.012 amu x 0.01991= 1.993 amu

For 11X: 11.009 amu x 0.8009 = 8.817 amu

For element X: atomic mass =10.810 amu

* Atomic mass of element X ?

*isotope 10X

mass = 10.012 amu

rel. abun= 19.91% or 0.1991

*Isotope 11X:

mass = 11.009 amu

rel. abun.= 80.09% or 0.8009

slide14

Practice

1. The element of copper has naturally occurring isotopes with mass number of 63and 65. The relative abundance and atomic masses are 69.2% for mass = 62.93 amu, and 30.8% for mass = 64.93 amu. Calculate the average atomic mass of copper

2. Calculate the atomic mass of bromine. The 2 isotopes of bromine have atomic masses and relative abundance of 78.92 amu (50.69%) and 80.92 amu (49.31%)

slide16

periods

Groups

1

2

3

4

5

6

7

8

9

10

11

12

13

14

15

16

17

18

1

2

3

4

5

6

7