Title: UNIT I: ALCHEMY
1UNIT I ALCHEMY
- SECTION II BASIC BUILDING MATERIALS
2COMPOSITION OF MATTER
- ALL MATTER IN THE UNIVERSE IS AN ELEMENT OR IS
MADE OF SOME COMBINATION OF ELEMENTS!
3ELEMENT
- Element- a unique substance that cannot be broken
down into simpler substances through chemical
processes. - Elements are the building blocks of matter.
- Elements are found on the periodic table.
- The first letter of an elements symbol is ALWAYS
uppercase and if there is a second letter it is
ALWAYS lowercase. - EX.
4COMPOUNDS
- Compounds- a pure substance that is a chemical
combination of two or more elements in a fixed
ratio. - Compounds are represented by chemical formulas.
- Compounds can be broken down into simpler stable
substances. - Ex.
5CHEMICAL FORMULAS
- Chemical Formula- a combination of symbols and
subscripts that indicates the number and types of
elements in a compound. - Ex. CuSO4
- Ex. Li2S
- Ex. NaCl
6Phases of Matter
- Matter can come in different physical forms
called phases. - Phase- the physical form a substance is in, such
as solid, liquid, or gas. - Phases are influenced by temperature.
- Solid (s), liquid (l), gas(g)
7Aqueous
- Aqueous- a substance that is dissolved in water.
- Aqueous (aq)
- What is the difference between Nacl(l) and
NaCl(aq)?
8Chemical Change
- Chemical Change- a change in which one or more
substances change into entirely new substances
with different properties. - Examples
9 Chemical Reactions
Chemical reaction- process by which one or more
substances change to produce one or more
different substances. Examples
10What are some indicators that chemical reaction
has taken place?
- Release/Absorption of Energy
11Products Reactants
Reactants-substances that exist prior to a
chemical reaction.
Products- substances that are formed as a result
of a chemical reaction.
carbon oxygen ? carbon dioxide
C (s) O2 (g) ? CO2(g)
reactants
product Carbon reacts with oxygen to form/to
yield carbon dioxide.
12Basic Laws of Matter
- Law of Conservation of Mass- mass is neither
created or destroyed during ordinary chemical
reactions or physical changes. - A B ? AB
- 1mu 3mu 4mu
Antoine Lavoisier
13History of the Periodic Table
- In 1869, Dmitri Mendeleyevs published the first
periodic table. - Mendeleev arranged the elements horizontally by
increasing atomic mass and placed elements in
groups (vertically) based on similar properties.
14History of the Period Table
- Mendeleyevs Periodic Table
15History of the Periodic Table
- Mendeleyevs Periodic Table
- Mendeleevs procedure left many holes throughout
the periodic table. - Mendeleyev was able to predict the properties of
elements that would eventually fill those holes
even though they were not discovered yet. - Ex. Ekasilicon- Germanium
16Average Atomic Mass
- Average Atomic Mass- the mass of one atom of a
given element measure in atomic mass units (amu). - Located beneath the elements symbol on the
periodic table. - Atomic mass units are extremely small units.
17History of the Periodic Table
- In 1913, Henry Moseley developed the Modern
Periodic Table. He arranged periodic table in
rows by increasing atomic number and in columns
by similar properties.
18History of the Periodic Table
- Moseleys Accomplishments
- Discovered that the positive charge of the
nucleus increases from one element to the next. - Led to the modern definition of atomic number.
- Moseleys periodic table explained some of the
contradictions that Mendeleev experienced within
his model.
19History of the Periodic TableEarly 1900s
Moseleys Periodic Table
20Atomic Number
- Atomic Number- Number of protons in an atom.
- Located above the elements symbol on the periodic
table.
21Periodic Law
- Periodic Law- states that the chemical physical
properties of the elements are periodic function
of their atomic numbers. - Group/Family- vertical columns of elements on the
periodic table with similar properties. - Periods- horizontal rows of elements on the
periodic table arranged by increasing atomic
number. -
22Metals, Nonmetals, Metalloids
- Metals
- Make up most of the periodic table.
- Ductile- can be drawn into wire
- Malleable- can be hammered into thin sheets.
- Lustrous- shiny
- Good Conductors of heat electricity
- Located to the left of the step ladder on the
periodic table.
23Metals, Nonmetals, Metalloids
- Nonmetals
- Brittle-break when hammered.
- Poor conductors of heat electricity.
- Lack luster
- Located to the right of the step ladder on the
periodic table.
24Metals, Nonmetals, Metalloids
- Metalloids
- Semimetals.
- Properties of both metals nonmetals.
- Located along the step ladder on the periodic
table. - Examples B, Ge, Sb, Te, At, Si, As, Po
25Metals, Nonmetals, Metalloids
26Alkali Metals- Group 1A
- Most reactive group of metals.
- Usually found in combined form as a salt due to
their high reactivity. - Combine vigorously with nonmetals especially
groups 6A 7A . - React readily with water.
- Soft and silvery appearance.
27Alkaline Earth Metals- Group 2A
- Found in the earths crust but not in the
elemental form due to their high reactivity.
They are usually found in rock structures. - 2nd most reactive group of metals.
- More dense than group 1.
- Shiny silvery-white color.
28Transition Metals- Groups 1B-8B
- Typical metallic properties.
- Good conductors.
- Lustrous.
- Produce colored ions.
29Main Group Elements Groups 1A-8A
- Properties of elements vary greatly.
- Contains all of the nonmetals metalloids as
well as some metals.
30 Halogens -Group 7A
- Most reactive groups of non-metals.
- React vigorously with metals (especially groups
1A 2A) to produce salts. - Fluorine is a poisonous pale yellow gas, chlorine
is a poisonous pale green gas, bromine is a toxic
and caustic brown volatile liquid, and iodine is
a shiny black solid which easily sublimes to form
a violet vapor on heating. - Found in nature in the combined state.
31 Noble Gases- Group 8A
- Least reactive of all elements.
- Often called inert gases.
- All are gases.
- The noble gases are all found in minute
quantities in the atmosphere, and are isolated by
fractional distillation of liquid air.
32Inner Transition Metals- Periods 6 7
- Lanthanides (Period 6)- Rare Earth Metals
- Shiny reactive metals
- Actinides (Period 7)
- Unstable radioactive metals.
- Most are laboratory made.
33Reactivity of Metals Trend
- Period Trend- Metals increase in activity from
right to left on the periodic table. - The alkali metals are the most reactive group of
metals. - Group Trend- Metals increase in reactivity from
top to bottom with a group. - Ra is the most reactive alkaline earth metal.
34Reactivity of Nonmetals Trend
- Period Trend- Nonmetals increase in activity from
left to right on the periodic table with the
exception of the noble gases. - The halogens are the most reactive group of
nonmetals. - Group Trend- Nonmetals increase in reactivity
from bottom to top with a group. - F is the most reactive halogen.
35Reactivity Trends
- What is the most reactive metal on the periodic
table? Explain. - Circle the most reactive nonmetal in each row
- Te Po S
- Br I Cl