Download Properties of Matter Power Point

Properties of Matter
Element
A pure substance that
cannot be broken
down into simpler
substances by
ordinary chemical
means.
Sulfur
Atom
The smallest unit of an
element that still has
the properties of that
element.
Each element on the
periodic table is
composed of atoms
of only one kind.
Compound
A substance made up
of atoms of more
than one element
bonded together.
Ex: H2O has different
properties than H or
O alone.
Water (liquid)
Oxygen (gas)
Molecule
The smallest unit of a
substance that still
has all of the
properties of that
substance.
A molecule can be
composed of atoms
of a single element
(N2), or be a
compound (H2O).
Nitrogen
Water
Chemical Formula
The chemical symbols and
numbers indicating the
numbers of atoms
contained in the basic
unit of a substance.
Ex: A water molecule
(H2O) contains two
hydrogen atoms and one
oxygen atom.
Chemical Formula
A glucose molecule
(C6H12O6) contains 6
carbon atoms, 12
hydrogen atoms, and
6 oxygen atoms.
States of Matter
States of Matter
Solid- A form of
matter with a definite
volume and a
definite shape.
States of Matter
Liquid- A form of
matter that has a
definite volume but
no definite shape.
States of Matter
Gas- A form of matter
that has no definite
volume and no
definite shape.
Melting Point
The temperature at
which a solid
becomes a liquid.
(0°C for water)
Boiling Point
The temperature at
which a liquid
becomes a gas.
(100°C for water)
How Do Solids Differ From Liquids?
Particles are closer together. (Greater density)
Particles have less energy. (Moving slower)
Attractive forces between molecules are
stronger.
How Do Liquids Differ From Gases?
Particles are closer together.
Particles have less energy.
Attractive forces between molecules are
stronger.
Early Ideas About The Atom
Democritus (Greek)Proposed the idea that
all matter is composed
of very small particles
that could not be
divided. Atom“indivisible”
Early Ideas About The Atom
John Dalton (b. 1766)Proposed the idea that
all matter is
composed of small
particles that
combine to form
molecules.
Dalton’s Atomic Theory
1. Every element is made up of tiny particles
called atoms that cannot be broken down into
simpler particles.
2. Atoms of the same element are exactly alike.
3. Atoms of different elements can join to form
molecules.
Early Ideas About The Atom
J.J. Thomson (18561940)- Proposed the
idea that atoms are
composed of smaller
charged particles that
hold the atom
together. Opposite
charges attract.
Early Ideas About The Atom
Ernest Rutherford
(1871-1937)- Conducted
an experiment that
provided evidence for
the existence of a
positively charged
nucleus inside of atoms.
The mass of an atom is
concentrated inside the
nucleus.
Early Ideas About The Atom
Niels Bohr (18851962)- Proposed the
idea that negatively
charged electrons are
located in orbits or
energy levels around
the nucleus.
Sub-atomic Particles
Nucleus- The center of an atom. Made up of
protons and neutrons.
Proton- A sub-atomic particle in the nucleus of
an atom. Protons have a positive electrical
charge (+) and a mass of 1 atomic mass unit
(amu).
Sub-atomic Particles
Neutron- A sub-atomic particle in the nucleus of
an atom. Neutrons are neutral, meaning that
they have no charge, and a mass of 1 amu.
Electron- A sub-atomic particle orbiting outside
the nucleus of an atom. Electrons have a
negative electrical charge and no mass.
Atoms in their most stable state have an equal
number of protons, neutrons and electrons.
Sub-atomic Particles
Mass
Charge
Location
Electrons
~0
-1
Orbits in
shells around
nucleus
Protons
1amu
+1
Nucleus
Neutrons
1amu
Nucleus
Atomic Number
The number of
protons in the
nucleus of an
atom.
Atomic Mass
The number of
protons and
neutrons in the
nucleus of an
atom.
Valence Electron
An electron in the
outermost energy
level of an atom.
Which Element?
(2,8,6)
Atoms are stable with 8 valence electrons
Ion
An atom or group
of atoms that has
lost or gained
electrons and is
left with a net
electric charge.
Chemical Bonding
The attractive force that holds atoms together
in molecules and compounds.
Ionic Bond
A chemical bond in which electrons are
exchanged between atoms.
Ex: Li+F−
Crystal Lattice
An orderly, three dimensional structure
produced by ions in an ionic compound.
Covalent Bond
A chemical bond in which electrons are
shared between atoms.
Ex: O2
Molecule
A neutral group of
atoms that are
joined together by
one or more
covalent bonds.
Polar Covalent Bond
A covalent bond in which the electrons
are not shared equally.
Ex: H2O
Water Molecule
Polarity
Non-polar Covalent Bond
A covalent bond in
which the
electrons are
shared equally.
Ex: O2
Metallic Bond
The attraction between
a positive ion and the
“sea of electrons”
that surrounds it.