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UNIT I: ALCHEMY

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UNIT I: ALCHEMY SECTION II: BASIC BUILDING MATERIALS Reactivity of Nonmetals Trend Period Trend- Nonmetals increase in activity from left to right on the periodic ... – PowerPoint PPT presentation

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Title: UNIT I: ALCHEMY


1
UNIT I ALCHEMY
  • SECTION II BASIC BUILDING MATERIALS

2
COMPOSITION OF MATTER
  • ALL MATTER IN THE UNIVERSE IS AN ELEMENT OR IS
    MADE OF SOME COMBINATION OF ELEMENTS!

3
ELEMENT
  • 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.

4
COMPOUNDS
  • 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.

5
CHEMICAL 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

6
Phases 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)

7
Aqueous
  • Aqueous- a substance that is dissolved in water.
  • Aqueous (aq)
  • What is the difference between Nacl(l) and
    NaCl(aq)?

8
Chemical 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
10
What are some indicators that chemical reaction
has taken place?
  • Precipitate Formation
  • Odor
  • Release/Absorption of Energy
  • Bubbles/Gas Production

11
Products 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.
12
Basic 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
13
History 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.

14
History of the Period Table
  • Mendeleyevs Periodic Table

15
History 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

16
Average 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.

17
History 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.

18
History 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.

19
History of the Periodic TableEarly 1900s
Moseleys Periodic Table
20
Atomic Number
  • Atomic Number- Number of protons in an atom.
  • Located above the elements symbol on the periodic
    table.

21
Periodic 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.

22
Metals, 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.

23
Metals, 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.

24
Metals, 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

25
Metals, Nonmetals, Metalloids
26
Alkali 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.

27
Alkaline 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.

28
Transition Metals- Groups 1B-8B
  • Typical metallic properties.
  • Good conductors.
  • Lustrous.
  • Produce colored ions.

29
Main 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.

32
Inner Transition Metals- Periods 6 7
  • Lanthanides (Period 6)- Rare Earth Metals
  • Shiny reactive metals
  • Actinides (Period 7)
  • Unstable radioactive metals.
  • Most are laboratory made.

33
Reactivity 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.

34
Reactivity 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.

35
Reactivity 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
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