Atomic Structure. Unit I
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1 Atomic Structure Unit I
2 Atoms are composed of 2 regions: Nucleus: the center of the atom that contains the mass of the atom Electron cloud: Atomic Structure region that surrounds the nucleus that d contains most of the space in the atom
3 What s in the Nucleus? TThe nucleus contains 2 of the 3 subatomic particles: Protons:(p+) positively charged subatomic particles Neutrons:(n o ) neutrally charged subatomic particles The number of neutrons can change.
4 What s in the Electron Cloud? The 3 rd subatomic particle resides outside of the nucleus in the electron cloud Electron:(e - ) the subatomic particle with a negative charge and relatively no mass
5 and
6 How do these particles interact? Protons and neutrons are compacted in nucleus. They accounts for most of the mass of the atom. The negatively charged electrons are small and have small mass but occupy a large volume (space) outside the nucleus.
7 How do the subatomic particles balance each other? In an atom: The #of protons = # of the electrons If 20 protons than 20 electrons are to balance the overall charge of the atom The neutrons have no charge; Neutrons do not equal the number of protons or electrons
8 How do we know the number of subatomic particles in an atom? Mass number(a) = the number of protons + neutrons in the nucleus. Atomic number(z): indicates the number of protons in an atom A Z
9 Determining the number of protons and neutrons Neutrons=(mass # - atomic #) = A - Z Ex: Ne has a mass number of 20 and an atomic number of 10 Protons = 10 Neutrons = 20-10= 10
10 What about the electrons? The electrons are equal to the number of protons So e - = p+ = atomic # Ex: He(Helium) has a mass # of 4 and an atomic # of 2 p+ = 2 n o = 2 e - = 2
11 Number Protons + Number of neutrons
12 Determine the number of subatomic particles in the following: Cl has a mass # of 35 and an atomic # of 17 p + = 17, n o = 18, e - = 17 (35-17=18) K has a mass # of 39 and an atomic # of 19 P + = 19, n o = 20 e - = 19 (39-19=20)
13 Rutherford s Model He discovered the nucleus and proposed that an atom is just like a miniature solar system, with electrons orbiting around a massive nucleus, and as mostly empty space, with the nucleus occupying only a very small part of the atom. The 3 rd ring can hold up to 18 e - The 4 th ring and any after can hold up to 32 e - The 1 st ring can hold up to 2 e - The 2 nd ring can hold up to 8 e -
14 Energy Levels of an Atom Number of Electrons in each level.
15 Valence Electrons
16 VALENCE ELECTRONS Why are they important? VALENCE ELECTRONS ARE RESPONSIBLE FOR FORMING BONDS BETWEEN ATOMS DURING A REACTION.
17 Types of bonding BONDS form when two or more atoms react together or when atoms try to reach stability. ATOMS will share valence electrons or exchange(give or take) valence electrons to make bonds: Covalent (Molecular) Bonds: Share electrons Ionic Bonds: One atom will give and the other will take an electron Metallic Bonds: Electron sharing within a metal. It is b/c of electrostatic forces.
18 Isotopes Atoms that have the same protons and electrons but A different number of neutrons. It will change the mass number of the atom. Ex: 3 Isotopes of Hydrogen
19 Hypothesis, Theory, Or Law? Hypothesis must be testable, repeatable, and relate to observation. PREDICT EVENT. If then because statements Theory based on observation, experimentation and reasoning Never completely proven, but modified continually.explains EVENT Law expression that reliably describes behavior of natural world. DESCRIBES EVENT
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