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Unit 1: Matter

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Mystery Fluid Video

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How is there a liquid that can be formed into shapes?

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What Makes A Good Model?

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Friday 8/25

�BW: What is matter? What do you know about matter? Write at least two sentences

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Key Idea

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Matter is anything that has ___________ and takes up ___________________

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What is a substance?

Matter exists as different SUBSTANCES – a single type of matter that has a specific composition and properties

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Sodium Chloride (Salt) - NaCl

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How do we tell substances apart?

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Q: How do we tell substances apart?�A: Their physical and chemical properties

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Key Idea

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A substance’s properties can always be explained by what is happening at the particle level

Put a pin in this for now…

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Monday 8/28

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BW: What do you think matter is made of?

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Pure Substances

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Pure Substances: Only one substance present

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Sodium Chloride (Salt) - NaCl

Iron - Fe

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Elements: Cannot be divided into simpler substances

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Iron - Fe

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Compounds: Made from elements chemically bonded together (Elements bond 🡪 Compound)

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Sodium Chloride (Salt) - NaCl

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Mixtures

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Mixture: More than one substance present

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Homogenous Mixture: Substances that are combined and completely mix

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Homogeneous Mixture – Bronze

  • Mixture of elements Copper (Cu) and Tin (SN), but these are NOT chemically bound together
  • Homogeneous because you can’t see the copper or tin
  • The copper and tin RETAIN THEIR INDIVIDUAL PROPERTIES in the mixture

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Heterogeneous Mixture: Substances that are combined together, but do not completely mix

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Element, Compound, or Mixture?

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Tuesday 8/29

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BW: Is the following image an example of an element, compound, homogeneous mixture, or heterogeneous mixture?

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Nitrous Oxide – “Laughing Gas”

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Periodic Table

  • What do you know? (Things you already know)
  • What do you notice? (Observations you make)
  • What do you wonder? (Questions you have based on the observation)

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Using Symbols Activity

What do the symbols on the periodic table tell us?

  • Become familiar with the names and symbols of the specific elements on the periodic table
  • Find symbols that can be put together to spell words
  • Notice how some names do not match the letters of the symbol

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Using Symbols Activity

Wrap Up

  • How many different words were you able to make from the element symbols?
  • Why do you think each element has a unique chemical symbol and name?
  • Which old world name did you find to be the most unusual?

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Wednesday 8/30

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BW: What are elements made of?

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Atom: the most basic building block of matter

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The Smallest Bit Activity

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The Smallest Bit

  • How many times were you able to cut the paper in half?
  • Do you think you would be able to get that small using tools other than scissors?
  • What does this tell us about the size of an atom?

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A Brief History of Atomic Theory

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“The fact of all things being made of matter is the greatest discovery in scientific history”

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How did we come to learn what we know about the atom?

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Democritus (400 BC)

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Everything is made of very small, indivisible particles

ATOMOS “UNCUTTABLE”

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Thursday 8/31

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BW: What did Democritus call his particle? Why did he call it that?

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John Dalton (1766 – 1844)

Experiments prove the following:

  1. All matter is made of atoms
  2. Atoms of a given element are identical and have unique properties from other elements
  3. Compounds are combinations of two or more atoms in DEFINITE PROPORTIONS
  4. Atoms can REARRANGE to form new compounds in chemical reactions

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Dalton (continued)

  1. Compounds are combinations of two or more atoms in DEFINITE PROPORTIONS

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  • Atoms can REARRANGE to form new compounds in chemical reactions

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Dalton’s Model

  • Atoms have different sizes and properties depending on the element

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JJ Thomson (1856 – 1940)

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Atoms are made up of electrons that have NEGATIVE CHARGE

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Thomson’s Atomic Model: Plum Pudding

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Ernest Rutherford (1871 - 1937)

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Famous Gold Foil Experiment

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Rutherford’s Atomic Model

“It was as if you fired a shotgun at a piece of tissue paper and the shells came back and hit you!”

  1. Atoms have a dense, positively charged center: NUCLEUS
  2. Electrons orbit the nucleus like a planet
  3. Most of an atom is EMPTY SPACE

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Niels Bohr (1885-1962): Where are the electrons?

Electrons move around the nucleus at specific orbits, each with different energy levels

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James Chadwick (1891 - 1974)

There is a neutral particle to STABILIZE the protons in the nucleus → NEUTRON

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An Almost Complete Atomic Model

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Tuesday 95

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BW: What does JJ Thomson’s plum pudding atomic model describe? What’s the analogy?

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Parts of an Atom

  • Protons (+)
  • Neutrons (N)
  • Electrons (-)

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Determining Identity: The Proton

  • All atoms of the same element have the same number of PROTONS
  • The amount of protons determines the IDENTITY of an atom
  • The number of protons is called the ATOMIC NUMBER
  • The PERIODIC TABLE is organized by atomic number (1 through 118)
  • If an atom is neutral, the number of protons EQUALS the number of electrons (THEY CANCEL OUT)

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Neutrons and Mass Number

  • In the nucleus, there are also NEUTRONS
  • Neutrons and protons both have a mass of approximately 1 amu
  • The mass number is the sum of the protons and neutrons in the nucleus
  • P + N = Whole Number

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Nuclide Symbol

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Wednesday 9/6

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BW: Provide the nuclide symbol and number of protons, neutrons, and electrons for the following element

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Nuclide Symbol:

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Protons:

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Neutrons:

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Electrons:

Atomic Model:

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Electrons By Shell

  • The first shell can contain up to: 2 electrons
  • The second shell can contain up to: 8 electrons
  • The third shell can contain up to: 32 electrons

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Nuclide Symbol Practice

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Proton, Neutron, Electron Practice

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Atomic Model Practice

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Monday 9/11

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BW: Create the atomic model for chlorine

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Identify the Element Practice

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The Arrangement of the Periodic Table

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Wednesday 9/13

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BW: Create an atomic model for Fluorine and Chlorine. Do you notice any similarities between the two?

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Why does the periodic table look the way it does?

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The story of Dmitri Mendeleev and the periodic table…

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Friday 9/15

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BW: What pattern did we see when we went down the periodic table in the same column?

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Periodic Table Structure Reading

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Monday 9/18

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BW: What did Mendeleev notice about elements that were in the same column (on top of each other?

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The Periodic Table

  • Today we know of 118 elements. Half of these were discovered in the last 150 years
  • The concept that elements are the foundation of matter is ancient

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Standardizing Elements

  • As the number of elements grew, the need for a STANDARDIZED way to represent them increased.
  • Abbreviations are ONE or TWO letters; if two, the second is lowercase
  • Origin of element abbreviation is not always English

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Before Mendeleev

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Dmitri Mendeleev (1834 - 1907)

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Lithium, Sodium, Potassium

Highly reactive metals

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Carbon and Germanium

Unreactive Non-Metals

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Carbon

Germanium

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Fluorine, Chlorine, Bromine

Colorful, Poisonous Gasses

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Fluorine

Chlorine

Bromine

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Neon, Argon, Krypton

Colorless, Unreactive Gasses

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Mendeleev’s Greatest Contribution: Periodicity

  • Properties of elements repeat in a PREDICTABLE pattern called PERIODICITY… but the pattern did not always work with the discovered elements…

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Mendeleev’s Gaps

Eventually, all of the ??? are discovered and match Mendeleev’s predictions perfectly

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Format of the Modern Periodic Table

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Key Definitions

  • The Columns on the periodic table are called GROUPS or FAMILIES
    • Elements in the same group/family share many CHEMICAL AND PHYSICAL PROPERTIES

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Key Definitions (continued)

  • The Rows on the periodic table are called PERIODS
    • The rows designate the number of SHELLS of electrons in the element
    • Remember that each orbit has a different ENERGY LEVEL

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What was Mendeleev’s strategy for organizing the elements?

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Elements sorted by properties

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Tuesday 9/19

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BW: What are groups and periods of a periodic table? What do elements in the same period have in common? What do elements in the same group have in common?

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Wednesday 9/20

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BW: What are the three major types of elements? What are some ways in which they are different?

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Key Definitions

  • Ductile: Can be drawn into thin wires
  • Malleable: Can be flattened (into sheets) without shattering
  • Conductors: can pass along heat and electricity well

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Grouping The Periodic Table Reading

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Thursday 9/21

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BW: Name as many of the groups/families as you can without looking at your notes.

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Why are the elements grouped in the way that they are?

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Key Definitions

  • The Columns on the periodic table are called GROUPS or FAMILIES
    • Elements in the same group/family share many CHEMICAL AND PHYSICAL PROPERTIES

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Group 1: Alkali Metals

  • Most reactive group in the periodic table
  • React with water and with oxygen in the air. Can cause violent explosions
  • They are found in nature ONLY combined with other elements

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Group 2: Alkaline-Earth Metals

  • Less reactive than alkali metals, but still very reactive
  • Have many uses: low-density materials for planes, found in your teeth and bones, found in chalk and cement

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Groups 3-12: Transition Metals

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Friday 9/22

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BW: What are some characteristics of Alkali Metals?

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Group 17: Halogens

  • Very reactive non-metals
  • Highly poisonous in gaseous state

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Group 18: Noble Gases

  • Have full outer electron shells making them highly unreactive
  • Difficult to detect (Mendeleev didn’t know about them)

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Hydrogen: In its own world

  • Most abundant element in the universe
  • Reacts with many elements
  • Highly reactive – it can be used as fuel for rockets

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Lanthanides and Actinides

  • Part of the transition metals
  • First row is lanthanides. Often mixed with other metals to strengthen them
  • Second row is actinides. All are radioactive and not found in nature, but created in laboratories

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Wednesday 9/27

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BW: What is matter? What is a substance?

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Physical and Chemical Properties

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Review: Particle Theory of Matter

  • All matter is made up of SMALLER PARTICLES (ATOMS)
  • These particles are CONSTANTLY MOVING, even when objects appear motionless

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What is a substance?

Matter exists as different SUBSTANCES – a single type of matter that has a specific composition and properties

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Sodium Chloride (Salt) - NaCl

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Q: How do we tell substances apart?�A: Their physical and chemical properties

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Key Idea

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A substance’s properties can always be explained by what is happening at the particle level

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*Can be observed with your senses

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Coke and Diet Coke Demo

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Why Does Diet Coke Float?

  • Diet Coke = Aspartame (200x sweeter than sugar)
  • Regular Coke = Sugar

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** All sodas are essentially carbonated water and sugar

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Density is the amount of matter (mass) packed into a certain volume

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Remember: what happens at the particle level explains a substance’s properties

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You have a 50 gram sample of Copper that has a volume of 5.58 cubic centimeters. What is the density of Copper?

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The density of gold is 19.3 g/cm^3. If you have a 32 g sample, what is the volume of your sample?

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You a 27 cubic meter sample of lithium. Lithium has a density of 0.534 g/cm^3. What is the mass of your sample?

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Monday 10/2

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BW: You have a 35 g sample of Chromium that has a volume of 4.86 cm^3. What is the density of Chromium?

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Tuesday 10/3

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BW: Which substance is more dense?

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Substance

Mass (g)

Volume (mL)

Density ( )

Hydrochloric Acid

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Manganese

101.64

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Layering Liquids Lab

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Why do we need to measure density at constant temperature?

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Diffusion Demo

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Diffusion

  • Particles move from high concentration to low concentration (spread out)
  • HOW FAST THE DIFFUSION OCCURS is caused by how particles in the substance move

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HOT WATER

COLD WATER

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Thermal Expansion (Diffusion)

  • When a substance’s temperature increases, its particles MOVE FASTER and SPREAD AWAY FROM EACH OTHER
  • Result: The substance expands (DENSITY DECREASES)

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What can you say about the bonds in solid copper (melting point = 1085 C) compared to solid plastic (melting point = 130 C)?

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Key Idea

  • The higher the melting point, the harder it is to BREAK BONDS in a substance

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  • Substances with higher melting points have STRONGER BONDS between atoms

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Wednesday 10/4

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BW: List as many physical properties as you can remember. What is a physical property?

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Chemical Properties

  • CHEMICAL PROPERTIES describe a substance’s ability to react to form new substances
  • They are only observable when TWO SUBSTANCES REACT
  • Ex: Baking soda and vinegar

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**Only observed when changing the identity of a substance

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Common Indicators of Chemical Reactions

  • Change in Color
  • Change in Temperature
  • Production of Odor
  • Evolution of Gas (formation of bubbles)
  • Precipitate (formation of solid)

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Common Misconception: Heating Up a Substance…

Physical or Chemical?

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If changing STATE → Physical

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If changing into SOMETHING NEW (reaction) → Chemical

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Chemical Property or Physical?

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You leave a copper pipe outside in the rain. When you go to bring it back in, you notice it has turned bluish-green in certain places. This is an example of a _________________ property.

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You cut a sample of gold in half and weigh it. It’s mass is a ___________ property.

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You boil water and it starts to evaporate into gas. This is an example of a ______________ property.

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You drop mentos into a 2L bottle of Coke and it shoots up a rocket of foam. This is an example of a ___________________ property.

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You melt lithium down into liquid form and notice that its density has decreased. This is an example of a ___________________ property.

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Chemical Properties Lab

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Universal Indicator

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Vinegar (Strong Acid)

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Acid + Base = Reaction

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Thursday 10/5

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BW: You boil some water and it starts to turn to vapor. Is this an example of a physical or chemical change?

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