Matter – ________________________________________.
Mass - the amount of matter an object has.- ___________________________. Gravity has an
impact on weight.- The same mass on the earth
would weigh less on the moon because less gravity on moon.
Elements – _____________________ – cannot be broken down into simpler types of matter. Examples: oxygen, carbon, hydrogen, and nitrogen – these four make up more than 90% of the mass of all living things!
Periodic Table :- Displays elements in an
organized manner.- From left to right – general
trend is toward larger sized atoms.
- See page 31 in textbook.
See page 31 in textbook:Atomic Number =
_____________________________.Atomic Mass =
______________________________________________________________________.Atom – ______________________________that
______________________________.
Atomic Structure consists of:
1. _________ = central core – consists of ______ (+) and _________ (0).
NOTE: #of protons or atomic number determines the atom’s identity.
2. _________ (-) orbit in energy levels or “shells” around the nucleus.
NOTE: # of protons = # of electrons to give an atom a net charge of zero.
3. 1st Shell (closest to nucleus) – holds 2 electrons (e-)…..these are the lowest energy electrons.
4. Each shell after the 1st can hold up to 8 electrons(e-)…..higher energy e-’s.
NOTE: In most elements, the outer shell is not filled. This determines the reactivity of the atom. See page 32 in textbook.
Compound – ______________________________________________. Exs.) water – H₂0, ammonia –
NH₃, glucose – C₆H₁₂O₆.
Isotopes – ______________________________________
________________________ it has.Ex.) C₁₂ and C₁₄ (radioactive and unstable)
Molecule – _____________________________________
_______________________________of the substance and can exist in a free state.
Exs.) O₂, O3 H₂O, CO₂, DNA, protein.See page 33 in book for bonding info:
Ionic Bonds:Ion = atom with a + or – charge from
_____________________________________.Ionic Bond – occurs when
______________________________________________. Ex.) NaCl – salt.
Energy – _____________or cause change. Energy can change forms. Ex.) electrical can change to radiant and thermal (light bulb).
Free Energy – energy available to do work.
__________________– solid, liquid, gas….depends on the motion of molecules. Ex.) Water – temperature makes molecules move at different rates and turns water to solid, liquid, or gas.
Energy and chemical reactions:CO₂ + H₂O ↔ H₂CO₃↑ ↑ ↑_________ __________
Activation Energy – energy needed to start a reaction. (see graph on page 37 in textbook).
Exergonic Reactions – involve a net ______________________________. Ex.) Sugar → CO₂ + water + energy.
Endergonic Reactions – involve a net _____________________________. Ex.) CO₂ + water + sunlight → sugar.
Catalyst – _______________________________________
____________________. Ex.) ENZYMES act as catalysts. (see enzyme deficiency on page 37 in textbook.
Reduction-Oxidation Reactions (REDOX reactions):
- Oxidation – reactant __________________and takes on a positive charge.
- Reduction – reactant __________________ and takes on a negative charge.
- Ex.) Na⁺ + Cl⁻ → NaCl (ionic bond)
Solution – a mixture in which _________________________________________…..can be liquids,
solids, or gases. Ex.) Blood = iron, water, oxygen, sugar, wastesSolute – a ____________________ in the solution.Solvent – a
_____________________________________.Concentration of Solution – the amount of
solute dissolved in a fixed amount of solution. Ex.) 2% saltwater = 2grams salt in 100ml water.
Saturated Solution – ____________________________________________________….the solution is
“saturated”.
Aqueous Solution – solutions in which _______________
_____________ …..very important to living things as we are made up of lots of different aqueous solutions. Exs.) blood, urine, lymph, spinal fluid, mucus.
Acids and BasesDissociation of Water – force of attraction
between water molecules cause them to break apart.
Pure water is neutral - # of OH⁻ and H₃O⁺ ions are equal.
Acid - ___________ions is greater than OH⁻ ions.
Ex.) Hydrogen chloride gas in water:
HCl ↔ H⁺ +Cl⁻ H⁺’s make the water acid.
Bases (Alkaline) - #of _________is greater than H₃O⁺ ions. Ex.) Sodium Hydroxide dissolved in water: NaOH ↔ Na⁺ + OH⁻ OH⁻ ions make the water basic or alkaline.
pH Scale – compares the relative concentrations of OH⁻ and H₃O⁺ in a solution.
pH – change in 1 pH unit = tenfold change in acidity/alkalinity. See figure 2-10, page 42 in book.
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