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

Slides:

Advertisements

Similar presentations

I. Subatomic Particles (p )

Advertisements

Section 4.3 How Atoms Differ

4.3: HOW ATOMS DIFFER ATOMIC NUMBER

Atomic Structure Nucleus – contains protons and neutrons

OF PROTONS, NEUTRONS AND ELECTRONS IN AN ATOM

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

ISOTOPES Chemistry. I. Why Atoms Differ? A. Atoms of different elements have their own unique structures 1. Because they have different structures they.

Atomic Structure I. Subatomic Particles.

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

Isotopes Atoms of the same element that different mass numbers

Chapter 18 Lesson 2 Masses of Atoms

Atoms and the Periodic Table

Atoms – The Basics. Inside the Atom  Atoms are made up of smaller particles  These particles are found in different regions of the atom.

More about isotopes Atomic mass vs average atomic mass or atomic weight.

 Atomic Number- the number of protons in the nucleus of an atom of that element  Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic.

Isotopes Atoms of the same element with different mass numbers. Mass # Atomic # Nuclear symbol: Hyphen notation: carbon-12 Courtesy Christy Johannesson.

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

C. Johannesson Atomic Structure. Structure of the Atom  Protons- Positively charged particles in the nucleus  Neutrons-neutrally charged particles in.

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.

Isotopic Abundance SCH 3U. Atomic Mass The mass of an atom (protons, neutrons, electrons) Relative Atomic Mass: An element’s atomic mass relative to the.

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.

Atomic Number & Atomic Mass

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

Atomic Structure The Periodic Table, Isotopes, and Average Atomic Mass.

Calculating Particles in a atom

Isotopes. The Nucleus  The number of protons in the nucleus of an atom is unique to each type of element  BUT, the nuclei of the same type of element.

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

Calculating Particles for an ion. Representations from the Periodic Table Fe Iron Oxidation States Name Atomic Mass Atomic Number.

LEARNING ABOUT ATOMS BY READING THE PERIODIC TABLE.

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

Atomic Mass. Atomic mass Most of the mass of an atom is in the nucleus. Most of the mass of an atom is in the nucleus. The nucleus is where all of the.

Chapter 4 AVERAGE ATOMIC MASS. Atomic Mass… n The weighted average of the masses of all the naturally occurring isotopes of that element. n Is not a whole.

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

Ch. 3 - Atomic Structure Subatomic Particles – show powers of ten ect…..

Ch. 3-3a Distinguishing and Counting Atoms. POINT > Define Atomic Number POINT > Define Mass Number POINT > Describe and identify isotopes POINT > Determine.

Ch. 3 - Atomic Structure Subatomic Particles.

1 The Atom Atomic Number and Mass Number Isotopes.

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

Same Element Different Atom- Isotopes All atoms of a particular element are not exactly alike. Some elements have atoms with different masses (isotopes)

Lesson 24: Isotopes An element can be identified by the # of protons it has # of neutrons can vary Neutrons add to the mass of the atom, but do not change.

Daily Science Who discovered the electron and how did he discover it? What was his model called? What tells you the number of p + an element has? Write.

I. From Philosophical Idea to Scientific Theory (p )

Calculating Atomic Mass

Ch. 3-3a Distinguishing and Counting Atoms

II. Masses of Atoms Mass Number

Now you try! Helium – 4 Oxygen – 16 Magnesium – 26 Isotope

Calculating Average Mass

Atomic Structure Subatomic Particles C. Johannesson.

Subatomic Particles Masses of Atoms Mass Number Isotopes Ions

III. Masses of Atoms (p ) Atomic Mass Mass Number Isotopes

The atom and Isotopes.

Ch Atomic Structure II. Masses of Atoms (p.30-31) Mass Number

Atomic Particles Particle Charge Mass # Location Electron -1

Atomic Structure.

Atomic Structure.

Mass of Individual Atoms

I. Atomic Structure II. Masses of Atoms Mass Number Isotopes Ion

Ch. 3 Atoms 3.3 Counting Atoms.

III. Masses of Atoms (p ) Atomic Mass Mass Number Isotopes

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.

III. Masses of Atoms (p ) Atomic Mass Mass Number Isotopes

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

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

III. Masses of Atoms Atomic Mass Mass Number Isotopes

I. Structure of the Atom Chemical Symbols Subatomic Particles

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

ARE ALL ATOMS OF THE SAME ELEMENT IDENTICAL?

Chapter 18 Lesson 2 Masses of Atoms

Presentation transcript:

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

A. Mass Number mass # = protons + neutrons always a whole number © Addison-Wesley Publishing Company, Inc. always a whole number NOT on the Periodic Table! C. Johannesson

B. Isotopes Mass # Atomic # Atoms of the same element with different mass numbers. Nuclear symbol: Mass # Atomic # Hyphen notation: carbon-12 C. Johannesson

B. Isotopes © Addison-Wesley Publishing Company, Inc. C. Johannesson

B. Isotopes Chlorine-37 atomic #: mass #: # of protons: # of electrons: # of neutrons: 17 37 20 C. Johannesson

C. Relative Atomic Mass 12C atom = 1.992 × 10-23 g atomic mass unit (amu) 1 amu = 1/12 the mass of a 12C atom 1 p = 1.007276 amu 1 n = 1.008665 amu 1 e- = 0.0005486 amu © Addison-Wesley Publishing Company, Inc. C. Johannesson

D. Average Atomic Mass Avg. Atomic Mass weighted average of all isotopes on the Periodic Table round to 2 decimal places Avg. Atomic Mass C. Johannesson

D. Average Atomic Mass EX: Calculate the avg. atomic mass of oxygen if its abundance in nature is 99.76% 16O, 0.04% 17O, and 0.20% 18O. Avg. Atomic Mass 16.00 amu C. Johannesson

D. Average Atomic Mass EX: Find chlorine’s average atomic mass if approximately 8 of every 10 atoms are chlorine-35 and 2 are chlorine-37. Avg. Atomic Mass 35.40 amu C. Johannesson