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Bohr Model of Atom

Borh Model of Atom

Democritus was a Greek philosopher (470-380 B.C) father of modern atomic. Term of atom.

Introduction

1

Marble or Solid Sphere

Dalton - 1803

- First that created atomic theory.

THEORY:

1) Atoms are tiny, indivisible particles.

2) Atoms of one element are all the same.

3) Atoms of different elements are different.

4) Compounds form by combining atoms.

2

Pudding

Thomson - 1904

- Discovered electrons.

- Atoms are composed of electron

troughout of a cloud of positive charge.

3

Nuclear

Rutherford - 1911

- Positive charge in the center: The NUCLEUS

- Discover protons.

- Experiment with gold foil (particles (+) went through).

4

Planetary

Borh - 1913

- Improved Rutherford's model.

- Electrons move around the nucleus in orbits (specific layer) of fixed sizes and energy.

5

Quantum Wave function

Schrodinger - 1926

- Electrons dont move in paths around the nucleus, but in WAVE.

- There is a "cloud of probability", called orbitals, which electrons are found.

James Chadwick

1932

- Discovered neutrons.

- Neutrons are also found in the nucleus.

6

Bohr Model of ATOM

Planetary Model

Examples

Bohr Model of ATOM

Bohr Model of ATOM

Protons and neutros are held tighly together at the center in a tiny, dense region called the NUCLEUS.

Electrons exist in the region around the nucleus in regular patterns called the

*Energy Levels/ Energy Shells

ATOM

ATOM

Neutral ATOM

Remember how a unit of electric charges can be defined????????

- Each proton has an electrical charge of ________.

- Each neutron has an electrical charge of ________.

- Each electron has an electrical charge of ________.

Recall that atoms are neutral (have an overall charge of zero.) This means that:

Number of protons = Number of electrons

EXAMPLES

EXAMPLES

Example 1:

C Carbon ATOM: 6 protons, 6 electrons

Example 2:

N Nitrogen ATOM: 7 protons, 7 electrons

Atomic Mass

Unit is defined as:

MASS OF 1 ATOM

A neutron has the same mass as a proton.

Atomic Mass

WHERE?

Atomic MASS

The mass of the atom comes mostly from the protons and neutrons in the nucleus.

The mass of the electrons is so small compared to the mass of the protons and neutrons it can be ignored.

Therefore: The atomic mass (or mass number) of an atom = NUMBER OF PROTONS + NUMBER OF NEUTRONS.

ISOTOPES

Why is the atomic mass an averaged decimal????

Because while atoms of the same element have the same number of PROTONS, they can differ in the number of neutrons.

This alters the mass of the atom.

Atoms that have the same number of protons but different number of neutrons, are called ISOTOPES of the same element.

EXAMPLES

Examples

C and C are isotopes found in nature. They both have 6 protons but C (with an atomic mass of 13 amu) has ___ neutrons while C (with an atomic mass of 12 amu) has ____ neutrons.

In nature, C is found as 99% and 1 % C. So the average atomic mass of the element C is calculated from that information to get a value of __________.

Putting all together

ATOMIC NUMBER= # of protons = # of electrons.

ATOMIC MASS= # of protons + # of neutrons.

This means:

- The number of neutrons

= Atomic mass- # of protons

= Atomic mass - atomic number

Putting ALL TOGETHER

Atomic Math

Atomic MATH

Oxygen Symbol:

Atomic Number:

Atomic Mass:

Protons:

Neutrons:

Electrons:

Lithium Symbol:

Atomic Number:

Atomic Mass:

Protons:

Neutrons:

Electrons:

Periodic Table

What information can you find in the periodic table?

- Period, group (1-18 or I-VIII) (family).

- Is organized in (3):

- The elements are arranged by increasing atomic number.

Periodic Table

Important families of the periodic table

Important families of the periodic table

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