States of Matter Notes

1
States of Matter

• States of Matter Notes
• There are four states of matter solid, liquid,
  gas, plasma.

2
Solids
States of Matter

• The particles of a solid are arranged in a
  definite pattern thus, a solid has both a
  definite shape and a definite volume.

• Solids are substances with densely packed
  particles. These particles may be ions, atoms, or
  molecules.
• Solids that have no crystal patterns are called
  glasses.

3
Solids and Liquids
States of Matter

• The atoms in solids vibrate close together at any
  temperature above absolute zero (2273C).

• The atoms in a liquid can then slide past each
  other.
• While liquids have a definite volume, they take
  the shape of their container.

4
Gases
States of Matter

• In gases, the particles are separated by
  relatively large distances and move about at
  extremely hibgh speeds.

• Gas particles move freely and independently of
  each other and travel randomly.
• Gases have no definite shape or volume and can
  expand into any space available, unless they are
  restrained.
• Earths gravity keeps the gases in the atmosphere
  from escaping into space.

5
Gases
States of Matter

• Individual particles in a liquid may gain
  sufficient energy to escape the liquid.

• Evaporation, or vaporization, is the process of
  changing from a liquid to a gas.

• When any liquid reaches its boiling point, it
  vaporizes quickly and becomes a gas.
• Sublimation is the slow change of state from a
  solid to a gas without an intermediate liquid
  state.

6
Plasma
States of Matter

• At temperatures greater than 5000C, the
  collisions between particles are so violent that
  electrons are knocked away from atoms.

• Such extremely high temperatures exist in stars,
  and, as a result, the gases of stars consist
  entirely of positive ions and free electrons.
• Plasmas are hot, highly ionized, electrically
  conducting gases.
• Plasmas can be found in neon tubes, lightening
  and the stars, including the sun!

7
Changes of State
States of Matter

• Solids melt when they absorb thermal energy and
  their temperatures rise.

• When a liquid absorbs thermal energy from the
  environment, it evaporates.
• When a liquid freezes, the same thermal energy is
  then released back into the environment.
• When a gas is cooled, it releases thermal energy
  in the process of condensation.
• Condensation is the change from a gas to a
  liquid.

8
Thermal Energy

• ____ ice melts
• ____ water vapor condenses to form rain
• ____ water freezes to make ice
• ____ water evaporates from a glass

9
Conservation of Matter and Energy
States of Matter

• The law of conservation of matter states that
  Matter cannot be created or destroyed but can
  change from one form to another.

• The law of the conservation of energy, also
  called the first law of thermodynamics, states
  that energy cannot be created or destroyed but it
  can be changed from one form to another.

10
Section Assessment
States of Matter

• 1. Match the following terms with their
  definitions.
• ___ crystalline structure
• ___ glasses
• ___ evaporation
• ___ sublimation

A. solids that consist of densely packed atoms
arranged at random B. a slow change from a solid
to a vapor without an intermediate liquid
state C. a solid in which the particles are
arranged in regular geometric patterns D. the
process of change from a liquid to a gas
C A D B
11
Section Assessment
States of Matter

• 3. Identify whether the following processes
  absorb or release energy into the environment.
• ___ condensation
• ___ evaporation
• ___ melting
• ___ freezing
• ___ sublimation

A. Absorb energy B. Release energy C. Neither
release or absorb
B A A B A
12
End of Section 3
13
Matter
What are elements?

• The physical world that surrounds you and all
  living things are composed of matter.

• Matter is anything that has volume and mass.
• On Earth, matter usually can be found as a solid,
  liquid, or gas.
• All matter is made up of elements.

14
What are Elements?
What are elements?

• An element is a substance that cannot be broken
  down into simpler substances by physical or
  chemical means.

• Currently there are 118 elements on the periodic
  table.
• Ninety-two elements occur naturally on Earth and
  in the stars.
• The other elements have been produced in
  laboratory experiments.

15
Elements
What are elements?

• Each element is identified by a one-, two-, or
  three-letter abbreviation known as a chemical
  symbol.

16
What Elements are Most Abundant?
What are elements?

• Silicon and oxygen make up 75 of earths crust.
• Al, Fe, Ca, Na, K, and Mg are also found.

17
Elements are Made of Atoms
What are elements?

• Each element has distinct characteristics.

• An atom is the smallest particle of an element
  that has all of the characteristics of that
  element.

• All atoms consist of even smaller particles
  protons, neutrons, and electrons.

18
Elements are Made of Atoms
What are elements?

• The nucleus, which is made up of protons and
  neutrons, forms the center of an atom.

• A proton (p) is a tiny particle that has mass
  and a positive electrical charge.

• A neutron (n0) is a particle with about the same
  mass as a proton, but it is electrically neutral
  that is, it has no electrical charge.
• Electrons (e-) are located outside the nucleus
  and have a negative charge.

• All atomic nuclei have a positive charge.

19
An atom of Helium

Atomic Number of 2 Atomic Mass of 4 -2 protons -2
electrons (To find neutrons- Mass-Atomic
) 4-22! -2 neutrons
20
Elements are Made of Atoms
What are elements?

• The number of protons and neutrons in different
  atoms varies widely.

• The mass number is the total number of protons
  and neutrons. It is the bottom number.

• The atomic number is the number of protons only
  in an atoms nucleus. This is the top number.
• The number of protons is ALWAYS equal to the
  number of electrons.
• You find the number of neutrons by subtracting
  the number of protons from the mass number.

21
Chlorine
22
Atomic Number Mass of Pros of Neutrons of Electrons Element Symbol
4 9 4 5 4 Be
45 21
31 Ga
65 30
20 Ca
24 12
37
W
49
23
Elements are Made of Atoms
What are elements?

• An energy level represents the area in an atom
  where an electron is most likely to be found.

• The mass of an atom depends mostly upon the
  number of protons and neutrons in its nucleus.
• The size of an atom depends upon the number and
  arrangement of its electrons.

24
Electrons in Energy Levels
What are elements?

• Electrons are distributed over one or more energy
  levels in a predictable pattern.

• Each energy level can hold only a limited number
  of electrons.

• The innermost energy level can hold only 2
  electrons.
• The second energy level can hold up to 8
  electrons.
• The third energy level can hold up to 18
  electrons.
• The fourth energy level can hold up to 32
  electrons.

• Electrons tend to occupy the lowest available
  energy level.

25
Isotopes
What are elements?

• The number of neutrons in the nuclei of an
  elements atoms can vary.

• Isotopes are atoms of the same element that have
  different mass numbers and the same chemical
  properties.

• The atomic mass of an element is the average of
  the mass numbers of the isotopes of an element.

26
Isotopes
What are elements?

• The nuclei of some isotopes are unstable and
  release radiation.

• Radioactivity is the spontaneous process through
  which unstable nuclei emit radiation.

• During radioactive decay, a nucleus can lose
  protons and neutrons, change a proton to a
  neutron, or change a neutron to a proton.
• Because the number of protons in a nucleus
  identifies an element, decay changes the
  identity of an element.

27
Section Assessment
What are elements?

• 1. Match the following terms with their
  definitions.
• ___ proton
• ___ energy level
• ___ neutron
• ___ atom

A. a tiny particle that has mass and a positive
electrical charge B. the smallest particle of
an element that has all of the characteristics of
that element C. a tiny particle that has mass
and is electrically neutral D. an area of an
atom where an electron is most likely to be
found
A D C B
28
End of Section 1
29
Compounds
How Atoms Combine

• A compound is a substance that is composed of
  atoms of two or more different elements that are
  chemically combined. (Ex. H2O)

• Most compounds have totally different properties
  from the elements of which they are composed.
• For most elements, an atom is chemically stable
  when its outermost energy level is full.
• Chemical bonds are the forces that hold the
  elements together in a compound creating a state
  of stability.

30
Compounds
How Atoms Combine

• Covalent Bonds

• One way in which atoms fill their outermost
  energy levels is by sharing electrons.
• A covalent bond is the attraction of two atoms
  for a shared pair of electrons that holds the
  atoms together.

31
Compounds
How Atoms Combine

• A molecule is composed of two or more atoms held
  together by covalent bonds.

• Molecules have no overall electrical charge
  because the total number of electrons equals the
  total number of protons.

32
Ions
How Atoms Combine

• Sometimes, atoms gain or lose electrons from
  their outermost energy levels.

• A charged particle called an ion is an atom that
  gains or loses an electron.

• In general, an atom in which the outermost energy
  level is less than half-full tends to lose its
  valence electrons.
• When an atom loses its valence electrons, it
  becomes positively charged and is indicated by a
  superscript plus sign.

33
Ions
How Atoms Combine

• An atom in which the outermost energy level is
  more than half-full tends to fill its outermost
  energy level by adding one or more needed
  electrons.

• Such an atom forms a negative ion which is
  indicated by a superscript negative sign.
• If the outermost energy level is exactly
  half-full, an atom may form either a positive or
  negative ion.

34
Ions
How Atoms Combine

• Ionic Bonds

• Positive and negative ions attract each other.
• An ionic bond is the attractive force between two
  ions of opposite charge.

• Positive ions are always written first in
  chemical formulas.

35
Metallic Bonds
How Atoms Combine

• In metals, the valence electrons are shared by
  all the atoms, in a metallic bond.

36
Chemical Reactions
How Atoms Combine

• Sometimes, compounds break down into simpler
  substances.

• A chemical reaction is the change of one or more
  substances into other substances.

• Chemical reactions are described by chemical
  equations.

37
Mixtures and Solutions
How Atoms Combine

• A mixture is a combination of two or more
  components that retain their identities.

• When a mixtures components are easily
  recognizable, such as soil, it is called a
  heterogeneous mixture. (Ex. Bag of M Ms)
• In a homogeneous mixture such as coffee, the
  component particles cannot be distinguished, even
  though they still retain their original
  properties.

38
Mixtures and Solutions
How Atoms Combine

• A homogeneous mixture is also called a solution.

• A solution may be liquid, gaseous, or solid.

• Seawater is a liquid solution consisting of water
  molecules and ions of many elements that exist
  on Earth.
• Air is a solution of gases, mostly nitrogen and
  oxygen molecules together with other atoms and
  molecules.
• Bronze is a solid solution of copper and tin
  atoms.

39
Mixtures and Solutions
How Atoms Combine

• Acids and Bases

• Many chemical reactions that occur on Earth
  involve solutions called acids and bases.

• An acid is a solution containing a substance that
  produces hydrogen ions (H) in water.

• The most common acid in our environment is
  carbonic acid, which is produced when carbon
  dioxide is dissolved in water by the following
  reaction. H2O CO2 H2CO3

40
pH Scale
41
Mixtures and Solutions
How Atoms Combine

• Acids and Bases

• The pH scale measures the hydrogen and hydroxide
  ions in solutions on a scale of 0 to 14, with 7
  being neutral.

• A solution with a pH reading below 7 is
  considered to be acidic.
• A solution with a reading above 7 is considered
  to be basic.

42
Section Assessment
How Atoms Combine

• 1. Match the following terms with their
  definitions.
• ___ covalent bond
• ___ compound
• ___ ion
• ___ acid

A. an atom that gains or loses an electron and
becomes electrically charged B. a solution
containing a substance that produces hydrogen
ions in water C. an attraction of two atoms for a
shared pair of electrons that hold the atoms
together D. a substance that is composed of atoms
of two or more different elements that are
chemically combined
C D A B
43
Section Assessment
How Atoms Combine

• 2. Identify whether the following are acidic,
  basic, or neutral.
• ___ Milk
• ___ Distilled water
• ___ Rainwater
• ___ Ammonia
• ___ Lemon
• ___ Tomato
• ___ Antacid

A. Acidic B. Basic C. Neutral
A C A B A A B
44
End of Section 2
45
Chapter Resources Menu
Chapter Resources Menu

• Study Guide
• Section 3.1
• Section 3.2
• Section 3.3
• Chapter Assessment
• Image Bank

46
Section 3.1 Main Ideas
Section 3.1 Study Guide

• The basic building blocks of matter are atoms.
  Atoms consist of protons, neutrons, and electrons.

• Protons have a positive electrical charge,
  electrons have a negative electrical charge, and
  neutrons are electrically neutral. Protons and
  neutrons make up the nucleus of an atom
  electrons surround the nucleus in energy levels.
• An element is a substance consisting of atoms
  with a specific number of protons in their
  nuclei. Isotopes of an element differ by the
  number of neutrons in their nuclei. Many elements
  are mixtures of isotopes.
• The number of electrons in the outermost energy
  levels of atoms determines their chemical
  behavior. Elements with the same number of
  electrons in their outermost energy levels have
  similar chemical properties.

47
Section 3.2 Main Ideas
Section 3.2 Study Guide

• Atoms of different elements combine to form
  compounds.

• Atoms held together by the sharing of electrons
  in covalent bonds form molecular compounds.
• Ions are electrically charged atoms or groups of
  atoms. Positive and negative ions attract each
  other and form ionic compounds.
• Acids are solutions containing hydrogen ions.
  Bases are solutions containing hydroxide ions.
  Acids and bases can neutralize each other.
• A mixture is a combination of components that
  retain their identities. A solution is a mixture
  in which the components can no longer be
  distinguished as separate. Solutions can be
  liquid, solid, gaseous, or combinations.

48
Section 3.3 Main Ideas
Section 3.3 Study Guide

• Matter on Earth exists in three common physical
  states solid, liquid, or gaseous. Matter in the
  universe includes plasma.

• Most solids have a crystalline structure.
• Liquids are densely packed arrangements of
  particles.
• Gases consist of widely separated, individual
  particles. Plasmas are hot, highly ionized,
  electrically conducting gases.
• Changes of state involve thermal energy.

49
Multiple Choice
Chapter Assessment

• 1. Which of the following is NOT about elements?
• a. They cannot be broken down into simpler
  substances by physical or chemical means.
• b. There are 47 naturally occurring elements
  on Earth and in the stars.
• c. All matter is made of elements.
• d. Each element is identified by a chemical
  symbol.

There are 92 elements that occur naturally on
Earth and in the stars.
50
Multiple Choice
Chapter Assessment

• 2. An elements atomic number represents ____.
• a. the number of protons in the atoms nucleus
• b. the combined number of protons and neutrons
  in the atoms nucleus
• c. the number of neutrons in the atoms nucleus
• d. none of the above

The combined number of protons and neutrons is
the elements mass number. The number of neutrons
can vary among the atoms of an element, creating
isotopes.
51
Multiple Choice
Chapter Assessment

• 3. Which is the most abundant element in the
  universe?
• a. oxygen c. iron
• b. helium d. hydrogen

Hydrogen makes up about 93.5 of all matter in
the universe. It is followed by helium at 6.3.
52
Multiple Choice
Chapter Assessment

• 4. Which is the most abundant element in Earths
  crust?
• a. hydrogen c. oxygen
• b. silicon d. aluminum

Oxygen makes up 46.65 of Earths crust. It is
followed by silicon (27.7), aluminum (8.1), and
iron (5.0).
53
Multiple Choice
Chapter Assessment

• 5. Which of the following is a molecule?
• a. argon c. nitrogen
• b. water d. uranium

Argon, nitrogen, and uranium are elements.
54
Short Answer
Chapter Assessment

• 6. What condition is necessary for matter to be
  ina plasma state?

The temperature must be greater than 5000ºC. At
temperatures this high, the collisions between
particles are so violent that electrons are
knocked away from atoms.
55
Short Answer
Chapter Assessment

• 7. What three forms can a solution take?

A solution may be liquid, gaseous, or solid.
56
Chapter 3 Images
Image Bank
57
Chapter 3 Images
Image Bank
58
Chapter 3 Images
Image Bank
59
Help
To navigate within this Interactive Chalkboard
product
Click the Forward button to go to the next
slide. Click the Previous button to return to the
previous slide. Click the Chapter Resources
button to go to the Chapter Resources slide where
you can access resources such as assessment
questions that are available for the
chapter. Click the Menu button to close the
chapter presentation and return to the Main Menu.
If you opened the chapter presentation directly
without using the Main Menu this will exit the
presentation. You also may press the Escape key
Esc to exit and return to the Main Menu. Click
the Help button to access this screen. Click the
Earth Science Online button to access the Web
page associated with the particular chapter with
which you are working. Click the Speaker button
to hear the vocabulary term and definition when
available.