Chapter 4: Section 1.  The Atom is the smallest particle of an element.

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Presentation transcript:

Chapter 4: Section 1

 The Atom is the smallest particle of an element

 The Atomic theory grew as a series of models that developed from experimental evidence. As more evidence was collected, the theory and models were revised.

 All elements are composed of atoms that cannot be divided

 All atoms of the same element are exactly alike and have the same mass. Atoms of different elements are different and have different masses

 An atom of one element cannot be changed into an atom of another element.

 Atoms cannot be created or destroyed in any chemical change, only rearranged ◦ Law of ____________ __ ____

 Every compound is composed of atoms of different elements, combined in a specific ratio

 Discovered that atoms had negatively charged particles and reasoned that the atom had to contain positively charged particles because the atom is electrically neutral 

 Inferred that an atom’s positive charge must be clustered in a tiny region in its center called a nucleus

 Electrons moved around the nucleus  He also named protons

 Theory came from Gold foil experiment. (see figure 4 & 5, pages 104 & 105)  some of the alpha particles had run into massive concentrations of positive charge and, since like charges repel, had been hurled straight back by them

 Showed that electrons could only have specific amounts of energy, leading them to move in certain orbits around the nucleus

 Electrons do not orbit the nucleus like planets, but can be anywhere in a cloud like region around the nucleus

 An electron’s movement is related to its energy level.  The specific amount of energy the electron has  Electrons of different energy levels are found in different places.

 James Chadwick discovered the neutrons, which are found in the nucleus, they have no charge and almost as much mass as the protons

 The model consists of an atom made up of a nucleus which contains the protons and neutrons surrounded by a cloudlike region of moving electrons contained in energy levels

 Protons are shown by a plus sign(1+), AMU = 1

 Electrons are shown by a minus sign(1-),  AMU = 1/ 1, 836

◦ Neutrons are shown by a zero sign(0), ◦ AMU = 1

 Every atom of an element has the same number of protons

 The atomic number identifies the element

 Since an element is electrically neutral, the atomic number also equals the number of electrons.

 The number of neutrons in an atom can vary.

◦ Atoms with the same number of protons but different numbers of neutrons are called isotopes. ◦ Figure 10, page 108

 An isotope is identified by its mass number

 The sum of protons and neutrons in the nucleus

◦ Number of neutrons can be found by subtracting the atomic number FROM the Mass number.  Mass number minus Atomic number = Neutron number