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Matter is anything that occupies volume (takes up space) and
has mass. A pure substance is matter that can no longer be
separated by a physical means. There are two types: 1.
elements and 2. compounds An element is made up of one
particular atom with the same atomic number. There are 103
different types of elements.
ATOMIC CHART
Symbols for elements
-Symbolized by 1-3 letters
Locatio
Particle
Charge
Mass
-Based on English or Latin name
n
-First letter capitalized, second letter lower case
C is for the element carbon.
Proton
Positive
1 Amu
Nucleus
Co is for the element cobalt.
CO is for the compound carbon monoxide.
Fe is for iron based on Latin name, ferum.
Neutron
Neutral
1 Amu
Nucleus
Atomic number – is the number of protons found in
the atom and determines what type of element a
1/1000
Electron
Electron Negativ
particular atom is.
e
Amu
Cloud
-Carbon always has 6 protons and the atomic
number of 6 but oxygen has 8 protons and the
atomic number of 8.
Atomic mass is the number of protons and neutrons found in the atom.
C-12 has 6P and 6N
C-14?
Isotopes – Two atoms with same number of protons but different number of neutrons. OR Two
atoms with same atomic number but different atomic mass. C-14 has 6P and 8N. * The extra 2N
makes C-14 radioactive.
If the number of electrons equals the number of protons the atom is said to be neutral.P = e, but if
they are unequal the atom is charged and called an ion. If the number of protons is greater than
the number of electrons the atom is a positive ion or cation. P > e
If the number of electrons is greater than the number of protons the atom is a negative ion or
anion. e > P
Electrons
-their mass is too small to be included in mass of atom.
-are found outside the nucleus in energy levels (the atom is mostly empty space).
-certain energy levels can only hold a certain number of electrons.
The 1st energy level can hold 2 electrons
The 2nd energy level holds a maximum of 8 electrons.
The 3rd energy level holds a maximum of 18 electrons
Atoms fill their energy level from the nucleus outward.
Hydrogen 1P, 1e
Carbon 6P, 6N, 6e Valence electrons are electrons found in the outer most energy level.
Carbon has 4 valence electrons. Sodium has 11 P, 12 N and 11 e
Draw the electron configuration
If an atom has 8 valence electrons, it is said to be stable, even if the energy level
can hold more (exception is when there is only one energy level then 2 valence electrons will
make is stable).
In order to achieve stability, atoms must either receive, transfer, or share electrons with other
atoms forming chemical bonds.
Types of Chemical bonds
Ionic Bond-Transfers electrons to form negative and positive ions attracted to one another.
Covalent Bond-Shares electrons to form a bond.
Hydrogen Bond-weak bond, attraction between H and another atom like oxygen.
Sodium is NOT stable, it has one valence electron it would like to get rid of.
Chlorine is NOT stable, it has one valence electron it would like obtain
In forming an ionic bond, sodium will transfer its one valence electron to chlorine making both
atoms stable. Now Na is positive and Cl is negative forming an attraction or ionic bond.
Covalent bonds involve the sharing of electrons. Consider oxygen and hydrogen. Neither is
stable,both want to receive electrons.
They form a covalent bond by sharing a pair of
electrons. Hydrogen is stable, but oxygen is not. It
shares with another H
Oxygen when it bonds with itself must share two
pairs of electrons Oxygen can not share just one
pair of electrons. It is must share two pairs of
electrons forming a double covalent bond. It is
usually drawn as
shown
When nitrogen bonds with itself, it
share three electron pairs, making a triple covalent bond
If there is unequal sharing of the electrons, the molecule
will have charges on it. It is called a polar covalent bond.
There is unequal sharing between
the oxygen and the hydrogen atoms
If there is equal sharing of the
electron pairs in a covalent bond then there is no net charge of the
molecule and it is said to be a nonpolar covalent bond. The carbon and
oxygen share their electron pairs equally. There is
no net charge on the molecule. A hydrogen bond is a weak bond
found between H and some other atom such as electronegatvie
atom such as O Hydrogen bonds are important in molecules such
as water, DNA, RNA and proteins.The hydrogen bonding found
BETWEEN water molecules gives water some unusual properties.
Properties of water-due to hydrogen bonding
1.Dissolves ionic and polar substances-Called universal solvent
2.High boiling point
3.High surface tension
4.High heat capacity-Absorbs a lot of heat energy before the temperature goes up. Energy
going into breaking hydrogen bonds, helps with evaporative cooling
5. Less dense as a solid. As a solid form more hydrogen bonds form. This increases the
volume making ice less dense than liquid water. This means that ponds freeze from the top
down. That layer on top of the pond becomes an insulator to prevent the ponds from freezing
solid.
In a chemical reaction, the atoms of some pure
substance are rearranged to form new pure
substances. Old chemical bonds must be
broken and new ones formed. During a chemical reaction, atoms cannot be created or destroyed,
just rearranged. This equation is not balanced.
Now the equation is balanced An acid is a
substance that when dissolved in water, it will
release a H+ ion. Not everything that contains
hydrogen is an acid. Ex. CH4 is methane gas
and not an
acid
A base is a substance that when dissolved in water, it will release a OH- ion. Not everything that
contains an OH is a base. Ex. CH3(OH) is methanol, an alcohol and not a base.