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Atoms & Periodic Table II
Interactions of Matter I
Interactions of Matter II
Vocabulary and Balancing Equations
Solutions, Acids, & Bases
100
Describe the arrangment of the periodic table (how elements are arranged, name the rows and columns).
Atoms are arranged from left to right in increasing atomic number. Groups are horizontal columns and periods are vertical rows.
100
State the positions of the reactants and products in a chemical reaction, along with their relationships.
The reactants are on the left, they combine to make the products, which are on the right.
100
State the three types of organic compounds.
What are: hydrocarbons, carbohydrates, and organic acids?
100
Explain what a metallic bond is.
A metallic bond has overlapping layers of electron shells.
100
State how concentration relates to a solution.
High concentration is when there is a high amount of solute per a set amount of solvent.
200
Describe the differences between covalent and ionic bonds.
Ionic bonds are stronger than covalent bonds, covalent compounds can bend without breaking, and do not typically conduct electricity. Ionic compounds are conductive in water, and are typically brittle.
200
State 5 signs that a chemical reaction has occured.
What is: change in properties, formation of precipitate, gas production, color change, release of energy, and absorption of energy?
200
Differenciate between endothermic and exothermic reactions.
Exothermic reactions release energy, and endothermic reactions absorb energy.
200
Balance this equation: C3H8 + O2 → H2O + CO2
What is: 2C3H8 + 10O2 → 8H2O + 6CO2
200
List the ways to increase the speed at which a substance will be dissolved.
What are: the introduction of motion, increase of solute surface area, and increase in temperature?
300
State the parts of an atom, their charges, and relative sizes.
The positive proton (1 amu), neutral neutron (about 1 amu), and negative neutron (1/1800 amu, or 1800 times less massive than proton and neutron).
300
State the ways to increase the speed of a chemical reaction.
What are: the introduction of a catalyst, increase in temperature, increase of surface area, and increase of concentration?
300
State how carbon is so versatile to bonding.
Carbon can bond very well because it has four valence electrons, which allows it to bond to itself and almost any other elements, allowing the formation of long repeating chains.
300
State which two substances will combine to form a covalent bond (metal, nonmetal, or metalloid).
What are two nonmetals?
300
State the relative differences between suspensions, colloids, and solutions.
Solutions are homogenous mixtures with small particles which do not scatter light or settle, colloids are heterogeneous mixtures with medium particles which scatter light but do not settle, and suspensions have large particles which settle and block light.
400
Draw a Bohr and dot diagram model of Nitrogen-14 (atomic number 7).
The Bohr model should have 7 neutrons and 7 protons in the nucleus, one ring with 2 electrons, and another ring with 5. The dot diagram model should be a capital N with 5 dots around it.
400
State the difference between full structural formulas and simplified structural formulas.
Full structural formulas give the exact position and arrangement of atoms, while simplified formulas only show how atoms generally bond.
400
Differenciate between polymers and monomers.
Monomers are groups of atoms which form repeating chains, which are polymers.
400
Define conductivity.
What is the ability to allow heat/electricity to pass through?
400
State how to calculate the concentration of a solution, and calculate the concentration of 2L of water and 4000g of sugar.
Divide mass of solute by volume of solvent, and 2000g/L.
500
State what a valence electron is and how it affects bonding.
What is the outermost electrons in an atom, and the amount of bonds is limited by the valence electrons?
500
Differenciate between chemical formulas and chemical equations.
Chemical formulas show the composition of a substance, while chemical equations use formulas to show a reaction.
500
State why chemical equations must be balanced.
Chemical reactions must be balanced because they must follow the Law of Conservation of Matter; matter (atoms) can neither be created or destroyed.
500
Balance this equation: CO2 + H2 → C2H6O + O2
What is: 2CO2 + 3H2 → C2H6O + 3O2
500
State what saturation with respect to a solution, and how to supersaturate a solution.
A saturated solution has the maximum amount of solute at a given temperature and pressure, and increasing temperature and pressure allows for a higher concentration.