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Topic 1.1 Matter & Change
EI: physical and chemical properties depend on the ways in which different atoms combine.
NOS: Making quantitative measurements with replicates to ensure reliability – definite and multiple proportions (3.1)
What is Matter?
What is Matter?
•Anything that takes up space and has mass.
– Made up of particles (atoms, molecules, ions)– Particles are in constant motion
A 2. States of Matter
State Shape VolumeDistance between particles
Arrangement of particles
Solid (S)
Fixed shape
Fixed volume
Close together regular
Liquid (l)
No fixed shape
Fixed volume
Close, but farther than solids
random
Gas or Vapor
(g)
No fixed shape
Not fixed Far apart random
Switching between states
• Solid melting Liquid
• Liquid freezing Solid
• Liquid evaporating (boiling) Gas
• Gas condensing Liquid
Switching between states
• Solid sublimation Gas
• Gas deposition Solid
Heat is required from solid to liquid to gas
Heat is removed from gas to liquid to solid
Switching between States
U1: Properties of Matter
Physical property• A characteristic of a substance
that can be measured or observed without changing the substance’s composition
Chemical property• The ability of a substance to
undergo a chemical reaction to form new substances
U1. Properties of Matter
Examples of Physical Properties
• Color• Solubility (Dissolving)• Odor• Hardness • Density• Melting Point• Boiling Point• State of matter• Thermal capacity• Mass
Examples of Chemical Properties
• Reactivity with oxygen • Reactivity with acids• Reactivity with bases• Reactivity with other
elements
Sodium and Chlorine Reaction
U1. Properties of Matter
Sodium is a silver metal at room conditions; combines with chlorine to make table salt; reacts with water to form hydrogen; has a density of 0.93 g/cm3; oxidizes rapidly in air, melts at 97.8oC.
• Using the above description, list the physical properties of sodium
• Using the above description, list the chemical properties of sodium
U1. Properties of Matter
Sodium is a silver metal at room conditions; combines with chlorine to make table salt; reacts with water to form hydrogen; has a density of 0.93 g/cm3; oxidizes rapidly in air, melts at 97.8oC.
• Using the above description, list the physical properties of sodium
• Using the above description, list the chemical properties of sodium
U1. Changes of Matter
Physical change• An alteration of matter that
does not change the chemical composition of the material.
U1. Changes of Matter
.
Chemical change• Results in a change in the
chemical composition of the substance(s). This is called a reaction.
U1. Changes of Matter
Examples of Physical Changes
• Freezing or melting• Boiling or condensing• Cutting• Grinding • Bending• Blending• Dissolving
Examples of Chemical Changes
• Combustion (burning)• Reacts with an acid• Reacts with a base• Rusting• Oxidizing• Decomposing• Digesting
U1. Changes of Matter Copy the statement on your paper and write P for
physical or C for chemical
1. Bending of a piece of wire
2. Burning of coal
3. Cooking a steak
4. Cutting grass
5. Sodium reacts with water
6. Iron rusts7. Silicon is insoluble in
water8. Ice melts9. Neon boils at -2460C10. Nitric Acid reacts
with Copper
U2. Distinguishing Compounds and Mixtures
• Elements are composed of just one type of atom. They cannot be separated into simpler substances using chemical means.
U2. Distinguishing Compounds and Mixtures
• Compounds are substances composed of two or more different kinds of atoms that have combined chemically. They can be separated by chemical means.
U2. Distinguishing Compounds and Mixtures
• Mixtures are a physical blend of two or more substances. They can be separated by physical means.
U2. Distinguish compounds and mixtures
• Elements– Represented by a chemical symbol (see Periodic
Table)
– Gold (Au), Iron (Fe), Oxygen (O or O2)
U2. Distinguish compounds and mixtures
Compounds– A fixed ratio of elements,
shown using element symbols and a number
U2. Distinguish compounds and mixtures
• Compounds– Examples:
• Water, H2O, contains 2 atoms of hydrogen (H) and one atom of oxygen(O).
• Salt, NaCl, contains one atom of sodium (Na) for each atom of chlorine (Cl).
U3. Mixtures
Mixtures: composition is not fixed• Homogeneous mixture- has uniform
composition and properties, also called solutions.– Ex: pure air, pure water, syrup
U3. Mixtures
Mixtures:• Heterogeneous mixture – non-uniform
composition, properties are not the same, able to see the separate components
• Ex: soup, concrete, granite
U3. Mixtures
• Ways to separate mixtures:– Heterogeneous: sieving, tweezers, skimming
– Homogeneous: distillation, ion exchange, reverse osmosis, evaporation
Distinguish between elements, compounds, and mixtures
Copy the item and indicate if it is an element, compound or mixture
1. Blood2. Hydrogen3. Brass (copper and zinc)
4. Ice (H2O)5. Motor oil
6. Silver
7. Orange juice
8. Neon
9. Sugar (C6H12O6)
10. Lake water
A& S. 1: Chemical Reactions
• In a chemical reaction, one or more substances change into new substances by rearranging the atoms
• Reactants Products
A& S. 1: Chemical Reactions
•Reactants ProductsReactants: the substances that are combined together
Products: the substances that are formed after the reactants are combined together.
A& S. 1: Chemical Reactions
Chemical Reaction Example:•Reactants Products
Copper+ nitric acid copper(II) nitrate+ nitrogen dioxide+water
Cu + HNO3 Cu(NO3)2 + NO2 + H2O
A& S. 1: Chemical Reactions
•Reactants Products
Copper+ nitric acid copper(II) nitrate+ nitrogen dioxide+water
Cu + HNO3 Cu(NO3)2 + NO2 + H2O
A&S 1. Chemical Reactions
A chemical reaction has occurred if:– Heat is absorbed or given off (change in
temperature)– Change in color or odor– Production of a gas or solid– Not easily reversible
A&S 1. Chemical Reactions
Law of Conservation of MassDuring any chemical reaction, mass is neither created nor destroyed, it is conserved.
– The mass of the products will always equal the mass of the reactants.
– The mass of each element is also unchanged.
A&S 1. Chemical Reactions
Law of Conservation of MassIn a reaction where hydrogen reacted with oxygen to produce water, if 4.5 g of hydrogen and 34 g of oxygen were used, how many grams of water were produced?
Hydrogen + oxygen = water4.5 + 34 = 38.5 g water