1. Matter: all matter is made up of
atoms.
is anything that has a
mass and a volume
all matter has a specific
density or arrangement
of atoms that can be used
to identify it.

2. John Dalton
(aka Jack)
1. Atoms are the smallest form of matter
2. Atoms make up all matter
3. Atoms of the same element are the same
4. Atoms cannot be broken down
5. Atoms combine in specific ratios

3. Thomson:
Discovered the electron
First model of atom

4. Rutherford:
Discovered presence of nucleus
And protons
Atom was mostly empty space

5. Chadwick:
Discovers the neutron

6. Bohr:
Suggested electrons move in energy
Levels
Presents model used today
(although not completely accurate)

7. M shell
L shell + n
K shell
nucleus

8. Electron cloud model
Electron cloud
Nucleus
Neutron
Proton

9. PERIODIC TABLE
Elements: roughly 88 naturally occurring
roughly 20 man made
organized arrangement
metals, nonmetals, metalloids, noble gasses
pure substance

10. Protons Positively charged Found in the nucleus Identifies element
Gives the element its atomic number
Gives nucleus its positive charge
Contributes to the atom’s reactivity +

11. Protons Positively charged Found in the nucleus Identifies element
Gives the element its atomic number
Gives nucleus its positive charge
Contributes to the atom’s reactivity +

12. ELECTRONS
Negatively charged
Found on the energy shells
Determines the reactivity of the atom
Has very small mass-not normally considered when calculating mass of atom. e

13. ATOMIC MASS: no. protons + neutron
-- ATOMIC NUMBER: no. protons
_________________________________
no. neutrons

14. Li At. Mass 7 -- At. # 3 4 Protons: 3 Neutrons: 4
___________________________ 4
Protons:
Neutrons:
Electrons: * *all unbonded atoms are electrically
and chemically neutral.
# of + = # of e.

15. Isotopes: Atoms of the same element that
Differ from each other by the number of
Neutrons.
Isotopes have the same Atomic number but
A different Atomic Mass.
45 known isotopes of iodine
I 127, I 136, 53
15 known isotopes of carbon
C 12, C 14, 6

16. Element – pure
Compound – 2 or more elements chemically combined
homogeneous
Mixture – 2 or more elements, compounds, or both physically combined.
homogenous or heterogeneous

17. Element – pure
Compound – 2 or more elements chemically combined
homogeneous
Mixture – 2 or more elements, compounds, or both physically combined.
homogenous or heterogeneous

18. Liquids: indefinite shape
definite volume
MA faster than solid
*MD larger than solid

19. Gas: Indefinite shape
Indefinite volume
MA fast Ma weak
MD large

20. MA, MD increased by increases in
Temperature = increases in energy.
Increases in MA and MD = changes
in state.

21. State changes are a result of increases
State changes are a result of increases* in thermal energy which directly increases* MD and MA. MA MD
Decrease
KE dec
condensation
vaporization MA MD
Increase
KE inc
melting
freezing

22. Bohr model Atomic mass = 7 Atomic number = 3 = 3 n = 4 e = 3 Lithium 3
= 3
n =
e = 3 3 + + n
Electron configuration:
2-1

23. Li F The outer most shell is called
the valence shell and is often unstable, meaning
It does not contain the octet number of electrons
In order for the atom to become stable or
Fill the shell to the octet rule, this shell will be
The one to bond.
Li F

24. Atoms that are not stable cause trouble –
they can be flammable, explosive, toxic.
These problems are what make an atom
reactive – meaning they want to become
stable.
Bonding:
Ionic loss or gain of electrons
Covalent sharing of electrons

25. IONIC BONDING: OCCURS BETWEEN-
METALS: LESS THAN 4 VALENCE ELECTRONS
AND
NONMETALS: MORE THAN 4 VALENCE ELECTRONS
***REMEMBER: ATOMS WANT TO USE LITTLE E!!
METALS WILL LOSE ELECTRONS
NONMETALS WILL GAIN THOSE ELECTRONS LOST

26. Ionic Bonding:
occurs between metal and nonmetal
> 4 val. e < 4 val. E
lose e gain e
form ions – charged atoms because
the # of protons does NOT
equal # electrons.
+ ion ion

27. - Na: metal, > 4 val. e, lose e F: nonmetal, < 4 val. e, gain e+ -
F: nonmetal, < 4 val. e, gain e
NaF sodium flouride

28. + -
Li2O

29. Bonding between atoms is a result of:
a. atoms need to be stable
b. atoms need to exist in a lower
energy state
c. attraction of positive nucleus and
negative electrons
d. size of the atom’s radius

30. COVALENT BONDING SHARING OF ELECTRONS ATOMS REMAIN NEUTRAL
OCCURS BETWEEN:
2 NONMETALS
A NONMETAL AND A METALLOID
HYDROGEN AND ALL NONMETALS
PRODUCES WEAK BONDS
PRODUCES COMPOUNDS THAT HAVE LOW MELTING POINTS
ALL ORGANIC COMPOUNDS ARE COVALENT

31. COVALENT BONDS Between hydrogen and A nonmetal Hydrogen has only one
Electron and therefore will never
Lose that electron. In order for
It to become stable and exist
In a lower energy state, it will
Share its only electron with
fluorine
Fluorine has 7 valence electrons
It needs 8 in order to exist in a lower
Energy state. It could bond ionically
With A metal or covalently with hydrogen
by sharing one of its valence electrons.

32. COVALENT BONDINGBETWEEN 2 NONMETALS
Nonmetals, because they have more than 4 valence electrons and
especially those that have small atomic radii, will bond with them-
selves in order to become stable and exist at a lower energy state.
These atoms will be called DIATOMS. There are 7 diatoms
That you will need to memorize. They are F, Cl, Br, I, O, N, H.

33. NONMETAL AND A METALLOID
COVALENT BONDING
BETWEEN
NONMETAL AND A METALLOID
Carbon will be our only metalloid with 4 valence electrons
Fluorine is a
Nonmetal with 7
Valence electrons
The resulting stable cmpd
Contains 4 F and 1 C. Because the atoms never LOST E’s they remain
neutral.

34. A NONMETAL AND A METALLOID HYDROGEN AND ALL NONMETALS
Comparison of bonds
Ionic Bonding:
occurs between metal and nonmetal
lose e gain e
form ions – charged atoms
COVALENT BONDING
SHARING OF ELECTRONS
ATOMS REMAIN NEUTRAL
OCCURS BETWEEN:
2 NONMETALS
A NONMETAL AND A METALLOID
HYDROGEN AND ALL NONMETALS

35. + POLARITY __ On polar molecules, electrons are controlled by one
UNEVEN DISTRIBUTION OF CHARGES + __
On polar molecules, electrons are controlled by one
Of the atoms.

36. Chemical and physical comparison
Physical properties
Chemical properties
Properties that describe the physical appearance of matter, such as size, shape, texture, density.
Properties can change and be returned to original properties.
Properties may be size dependent or size independent.
Properties describe the chemical composition of the matter, such as the elements that are bonded and the specific ratio; H2O, Fe2O3.
Chemical properties do not change without changing the composition of matter.
Properties are not affected by size.

37. Chemical and Physical changes
Chemical Changes
The changes affect the way the matter appears; size, color, shape.
These changes can be reversed.
The properties of the new matter are the same as the original.
The changes affect the appearance of matter.
The changes change the chemical composition of the matter.
These changes cannot be reversed.
The properties of the new matter are different than the original.