Transcript ESChap3MatterAtomicStructure

Matter and
Atomic Structure
Chap. 3
• What are elements?
• How atoms combine
• States of matter
What makes a gold
atom different from
a silver atom?
What are elements? – 3.1
Objectives
• Describe the particles
within atoms and the
structure of atoms
• Relate the energy
levels of atoms to the
chemical properties of
elements
•Define the concept of
isotopes
I. Element
Element
Substance that cannot be
broken down into simpler
substance by physical or
chemical means.
I. Element
A. Element names
Carbon
6
C
12.011
I. Element
A. Element names
B. Element symbols
Carbon
6
C
12.011
I. Element
A. Element names
B. Element symbols
C. Elements are made of
atoms
II. Atoms
Atom
Smallest particle of an
element.
II. Atoms
A. Composed of 3 particles
II. Atoms
A. Composed of 3 particles
1. Protons
II. Atoms
A. Composed of 3 particles
1. Protons
2. Neutrons
II. Atoms
A. Composed of 3 particles
1. Protons
2. Neutrons
nucleus
II. Atoms
A. Composed of 3 particles
1. Protons
2. Neutrons
3. Electrons
II. Atoms
A. Composed of 3 particles
B. Atomic number
Atomic number
Number of protons.
proton
neutron
Atomic number
Number of protons.
proton
neutron
5
II. Atoms
A. Composed of 3 particles
B. Atomic number
C. Mass number
Mass number
Sum of the number of
protons and neutrons
proton
neutron
Mass number
Sum of the number of
protons and neutrons
proton
neutron
11
II. Atoms
D. Electrons in Energy Levels
Electron Energy Levels
Energy level
First
Second
Third
Fourth
Electron Capacity
2
8
18
32
Model of Oxygen
Self Check – Ex. 1
Draw a model of the
lithium-7 atom. Include
protons, neutrons, and
electrons.
Self Check – Ex. 2
Draw a model of the
chlorine-35 atom. Include
protons, neutrons, and
electrons.
II. Atoms
D. Electrons in Energy Levels
1. Core electrons
II. Atoms
D. Electrons in Energy Levels
1. Core electrons
2. Valence electrons
Valence electron
Outermost electron found
in a shell.
III. Isotopes
Isotopes
Atoms with the same
number of protons, but
different numbers of
neutrons.
III. Isotopes
A. Isotopes have different
masses
III. Isotopes
A. Isotopes have different
masses
B. Nature contains a variety
of isotopes
III. Isotopes
A. Isotopes have different
masses
B. Nature contains a variety
of isotopes
C. Isotopes used to find
atomic mass of element
Atomic mass
The average of the masses
of each isotope present for
a give element.
III. Isotopes
D. Radioactivity
Radioactivity
The spontaneous decay of
an atom’s nucleus into a
new nucleus.
IV. Abundance
A. In Universe
Abundance in Universe
IV. Abundance
A. In Universe
B. In Earth’s crust
Abundance in Earth’s Crust
The End
How atoms combine – 3.2
Objectives
• Describe the chemical
bonds that unit atoms to
form compounds
• Relate the nature of
chemical bonds that hold
compounds together to
the physical structures of
compounds
•Distinguish between
different types of mixtures
and solutions
I. Compounds
Compound
More than one element
chemically combined.
I. Compounds
A. Covalent compounds
share electrons
I. Compounds
A. Covalent compounds
share electrons
1. Sharing electrons helps atoms
get full electron set
I. Compounds
A. Covalent compounds
share electrons
1. Sharing electrons helps atoms
get full electron set
2. Sharing may not be equal: this
makes polar molecules
I. Compounds
B. Ionic compounds transfer
electrons
I. Compounds
B. Ionic compounds transfer
electrons
1. When an atom gains an
electron it becomes _______
I. Compounds
B. Ionic compounds transfer
electrons
1. When an atom gains an
electron it becomes _______
2. When an atoms loses an
electron it becomes _______
Ion
An atom that has gained
or lost an electron.
I. Compounds
B. Ionic compounds transfer
electrons
1. When an atom gains an
electron it becomes _______
2. When an atoms loses an
electron it becomes _______
3. Opposites _______
I. Compounds
C. Metallic bonds have a ‘sea
of electrons'
II. Reactions
II. Reactions
A. Bonds are broken and
reformed
II. Reactions
A. Bonds are broken and
reformed
B. New substances are
formed
II. Reactions
A. Bonds are broken and
reformed
B. New substances are
formed
C. Energy is exchanged
III. Mixtures
III. Mixtures
A. Most mixtures are
heterogeneous
Heterogeneous
A mixture with visibly
different parts.
III. Mixtures
A. Most mixtures are
heterogeneous
B. Mixtures that are
homogeneous are called
solutions
Homogeneous
A mixture with the same
makeup throughout.
IV. Acids & Bases
IV. Acids & Bases
+
A. An acid makes H ions
IV. Acids & Bases
+
A. An acid makes H ions
B. A base produces OH ions
IV. Acids & Bases
+
A. An acid makes H ions
B. A base produces OH ions
C. The pH scale tells how
acidic/basic something is
The pH Scale
0 1
acidic
3
5
7
9
neutral
11
13 14
basic
The End
States of Matter – 3.3
Objectives
•Describe the states of
matter on Earth
• Explain the reasons that
matter exists in these
states
• Relate the role of
thermal energy to changes
of state in matter
I. The Four Phases of Matter
I. The Four Phases of Matter
A. Solid
I. The Four Phases of Matter
A. Solid
1. solids with regular structure
are described as crystalline.
I. The Four Phases of Matter
A. Solid
1. solids with regular structure
are described as crystalline.
2. in some solids there is no
organized pattern. These are
amorphous.
I. The Four Phases of Matter
A. Solid
B. Liquid
I. The Four Phases of Matter
A. Solid
B. Liquid
C. Gas
I. The Four Phases of Matter
A. Solid
B. Liquid
C. Gas
1. gases have undergone
vaporization or sublimation
Evaporation
Changing from liquid to
vapor
Sublimation
Changing from solid to
vapor
I. The Four Phases of Matter
A. Solid
B. Liquid
C. Gas
1. gases have undergone
vaporization or sublimation
2. gas particles are separated by
large distances
I. The Four Phases of Matter
A. Solid
B. Liquid
C. Gas
D. Plasma
Plasma
Hot, highly ionized,
electrically conducting
gas.
II. Changes in State
II. Changes in State
A. When a liquid changes to
a gas, heat is _______.
II. Changes in State
A. When a liquid changes to
a gas, heat is _______.
B. When a gas changes to a
liquid, heat is _______.
The End