Mass Spectrometer.

Slides:

Advertisements

Similar presentations

Reviewing Subatomic Particles

Advertisements

Atomic Structure Nucleus – contains protons and neutrons

Atoms 8.5A The student is expected to describe the structure of atoms, including the masses, electrical charges, and locations, of protons and neutrons.

Components of the Atom Nucleus: Nuclear Forces:

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

Atomic Structure I. Subatomic Particles.

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

STRUCTURE OF THE ATOM.

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

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.

1. Proton 2. Neutron 3. Electron 1. Protons 2. Neutrons 3. Electrons.

Atomic Mass. Masses in amu Only carbon-12 has an atomic mass exactly equal to its mass # One atomic mass unit (amu) is defined as 1/12 the mass of a carbon-12.

Mass Spectrometer.

Protons, Neutrons, and Electrons

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.

Atomic Structure: Atoms and Isotopes GPS 5. Simplified Model of the Atom Nucleus – the center of the atom that contains protons and neutrons Electron.

Parts of the Atom.

Atomic Structure Notes

Atomic Structure Current Atomic model

Section 2 Protons, neutrons, and electrons- how atoms differ

How Atoms Differ.

Atomic Structure Modern Atomic Theory.

The Modern View of Atomic Structure

Counting Atoms.

Calculating Average Mass

Atomic Structure Concepts.

Atomic Structure I. Subatomic Particles C. Johannesson.

Atomic Structure Subatomic Particles C. Johannesson.

Atomic Structure Notes

Atomic Structure/ Sub-particles- Definitions Mass Spectrometer

ELEMENTS, IONS AND ISOTOPES

STRUCTURE OF THE ATOM.

Atoms / Elements •Different number of protons

Atomic Structure Nat

The Atom CHAPTER 26.

Structure of the Nucleus – Outcomes

Atomic Particles Particle Charge Mass # Location Electron -1

Distinguishing Between Atoms

Atomic Structure.

# of Subatomic particles Atomic Mass - calculate

Ch. 4/5 Notes Day 3 1/28/16.

Foldables: Atoms Terms.

Elements, Isotopes and More

Bell Ringer List all elements in Column 18 and their symbol.

Intro to Atomic Structure

Isotopes Atoms with SAME number of PROTONS (atomic number) but DIFFERENT numbers of neutrons (i.e. mass number) 6 protons 6 neutrons 6 protons 7 neutrons.

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

The Structure of an Atom

e- p+ n0 0 amu 1 amu 1 amu Electron proton Neutron

How We Know What We Can’t See Looks Like Day 4 Average Atomic Mass

How We Know What We Can’t See Looks Like Day 2

The Atom Unit 2 Topic 1.

ATOM COMPOSITION The atom is mostly empty space

Atomic Structure Protons- positively charged, found in nucleus

Atomic Structure Nucleons Atomic Number

Do Now Write the following definitions: Proton: Neutron: Electron:

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

How We Know What We Can’t See Looks Like Day 4 Average Atomic Mass

Atomic Structure Nucleus Protons Neutrons Electrons.

A simple model of the atom.

Quantifying atoms and Molecules

Parts of the Atom.

Example Example 1: The atom of an element has a mass number of 214 and an atomic number of 82. a) How many protons and neutrons does it have? The number.

Atomic Particles Particle Charge Mass (kg) Location Electron -1

Presentation transcript:

Mass Spectrometer

The Mass Spectrometer and Atomic Mass * The actual mass of atoms was not known until the invention of the mass spectrometer. * In a mass spectrometer, ions of high mass deflect less than those of low mass. * If the charge of the particle is known, then the mass of the particle can be calculated.

Atomic Terms Atomic Mass Unit (amu): exactly equal to 1/12 of the mass of a carbon-12 atom. (1.9927 x 10-23g) 1 amu = 1.6606 x 10-24g) Isotopes: Atoms of an element having different atomic masses. Atomic Mass: The average relative mass of the isotopes of an element compared to the mass of carbon – 12.

Composition of the nucleus Atomic Masses Atomic mass is the average of all the isotopes of that element. Carbon = 12.011 Isotope Symbol Composition of the nucleus % in nature Carbon-12 12C 6 protons 6 neutrons 98.89% Carbon-13 13C 7 neutrons 1.11% Carbon-14 14C 8 neutrons <0.01%

Isotope Isotopic mass (amu) Abundance (%) 6329Cu 62.9298 69.09 6529Cu 64.9278 30.91 Atomic mass is then calculated in the following way: (62.9298)(0.6909) = 43.48 (64.9278)(0.3091) = 20.07 63.55

Particle Symbol Relative Electric Charge Relative Mass (amu) Actual Mass (g) Electron e- -1 1/1837 9.110 E-28 Proton p +1 1 1.673 E-24 Neutron n 1.675 E-24

The Atomic Scale Most of the mass of the atom is in the nucleus (protons and neutrons) Electrons are found outside of the nucleus (the electron cloud) Most of the volume of the atom is empty space “q” is a particle called a “quark”

About Quarks… Protons and neutrons are NOT fundamental particles. Protons are made of two “up” quarks and one “down” quark. Neutrons are made of one “up” quark and two “down” quarks. Quarks are held together by “gluons”