Chemistry Semester 1 Final Exam Review

Chemistry Semester 1 Final Exam Review

Chemistry Semester 1 Final Exam reviewName______per_____

  1. What is a definition of Chemistry?
  2. Matter includes all of the following EXCEPT:

a. air b. light c. smoked. water vapor

  1. What are two factors that distinguish matter?
  2. Define a physical change. ______Define a chemical change. ______Label which are physical changes and chemical changes:

a. peach spoils_____ b. copper bowl tarnishes______c. bracelet turns wrist green_____ d. glue gun melts a glue stick____

  1. The particles in a solid are

a. packed closely together b. constantly in motion c. very far apartd. able to slide past one another

  1. Physical means may be used to separate ______and they include ______, ______, ______, ______

Of the following groups, 1, 2, 14, 15, 17, 18:

  1. Group(s) ______contains only metals
  2. Group (s)______is called a Noble gases
  3. Group(s) ______has 7 electrons on the valence shell
  4. Group(s) ______needs to gain 3 electrons to fill a stable octet
  5. Group(s) ______a 2+ ion
  6. Group(s) ______has an electron dot notation of X
  7. Using the periodic table, an element similar to carbon would be______
  8. Based on their location on the periodic table, you could infer that ______is very unreactive
  9. The horizontal row on the periodic table is called a(n)______
  10. The vertical column of blocks on the periodic table is called a(n)______
  11. The elements on the zigzag line in the periodic table are ______
  12. Which is NOT a property of metal?

a. malleability b . unreactive c. ability to lose electronsd. ability to conduct heat

  1. The validity of scientific concepts is evaluated by

a. collecting factsc. voting by scientists

b. providing explanationsd. testing hypotheses

  1. All but one of these units are SI base units. The exception is

a. kilogram b. secondc. literd. Kelvin

  1. The symbol for the metric unit used to measure mass in the Chemistry lab is

a. m b. mmc. g d. L

  1. The quantity that describes the concentration of matter is

a. weightb. densityc. volumed. mass

  1. Convert: a) 2.5 liters into mL______b) 6.2 x 104 microliters to Liters______c) 0.5 kg to g ______
  2. A volume of 1 cc (cm3) is the same as ______mL
  3. To determine density, the quantities that must be measured are ______and ______
  4. The relationship between the mass m of a material , its volume V, and its density D is

a. V = mDb. Vm = D c. DV = md. D + V = m

28. The density of aluminum is 2.70 g/cm3. The volume of a solid piece of Aluminum is 1.50 cm3. Find the mass

  1. The density of pure diamond is 3.5 g/cm3. The mass of a diamond is 0.25 g. Find the volume
  2. What statement about density is true?
  1. two samples of a pure substance may have different densities if they are different sizes
  2. the density of a sample depends on its location on Earth
  3. a cylinder is always used to measure the volume
  4. density is a physical property that remains constant for a pure substance
  1. The number of grams equal to 0.5 kg is ______
  2. 30oC = ______K
  3. A measurement that closely agrees with accepted values is said to be ______(accurate or precise)
  4. In Chemistry, the quantitative labs need to have a confidence level of ______
  5. The equation for percent error is ______
  6. Calculate the percent error if you found the density of water to be 1.08 g/ml and the actual density of water is 1.0g/ml.
  1. Calculate the average atomic mass of an element with two isotopes. One isotope has a mass of 45 amu and an abundance of 44%. The second isotope has a mass of 44 amu and a relative abundance 56%.
  1. The variable that you change in the lab is the ______variable. The variable that responds to the change is called the ______variable. All other things do not change and are called ______
  2. At first Dalton thought the atom was ______, then Ruther ford discovered the ______of the atom, then the subatomic particles ______, ______, and ______were discovered
  3. The positively charged particle is the ______found in the ______of the atom
  4. The subatomic particle that has about the same mass as the proton, but with no electrical charge, is called a ______and is found in the ______of the atom
  5. The ______is negatively charged and is found in the ______of the atom
  6. ______is the person credited with placing electrons on levels and ______established the electron cloud theory.
  7. The forces that hold the particles together in the nucleus are ______forces
  8. Isotopes are atoms of the same element that ______
  9. All isotopes of hydrogen contain ______
  10. What is the atomic number for Nitrogen? ______To what subatomic particle does this correspond?
  11. Zinc –66 has ______protons and ______neutrons
  12. The number of atoms in 1 mole of carbon is ______
  13. The mass of 1 mole of Chromium is ______
  14. The mass of 3.5 moles of silicon is ______
  15. What is the electron configuration for sodium? Chlorine? Neon?
  16. What is the dot notation for magnesium? Bromine? Argon?
  17. How many electrons is each element trying to achieve in the valence level?
  18. Who is given credit with developing the modern periodic table? ______How was it arranged?______
  19. Which family is entirely radioactive?
  20. Which family will gain two electrons to complete their octet?
  21. Where are the transition metals located? What is special about their electron configuration that gives them special properties?
  22. As you move left to right across a period on the table the size (radius) ______
  23. As you move down a column(group) the ionization energy ______
  24. The most active metal is ______and the most active nonmetal is ______
  25. As atoms bond with each other, they

a. increase their potential energy, thus creating less-stable arrangements of matter

b. decrease their potential energy, thus creating less-stable arrangements of matter

c. increase their potential energy, thus creating more-stable arrangements of matter

d. decrease their potential energy, thus creating more-stable arrangements of matter

75. When atoms share electrons, a ______bond is formed

  1. When ______electrons are shared a triple covalent bond is formed
  2. Covalent bonds may be equally shared called ______and unequally shared called ______
  3. The most common example of an unequally shared covalent material is ______
  4. Define ionic bond and metallic bond.
  5. What are characteristics of a covalent bond, an ionic bond and a metallic bond (list on another paper)
  6. What is an exothermic reaction? ______What is an endothermic reaction?______
  7. Changing a subscript in a correctly written chemical formula
  1. changes the number of moles represented by the formulab. changes the charges on the other ions in the compound
  1. changes the formula so that it no longer represents that compoundd. has no effect on the formula
  1. Technetium-99 has been used as a radiographic agent in bone scans (9943Tc is absorbed by bone). If 9943Tc has a half-life of 6.0 hours how much of a 100µg sample would remain in the patient’s body after 2.0 days?
  1. Silicon-31 has a half-life of 2.5 hours. If we begin with a sample containing 1000mg of Si-31 how much will remain after 10 hours?
  1. What are α, β, γ particles?
  2. Rank α, β, γ radiation in order of increasing energy (from lowest to highest).
  1. 3717Cl → 3718Ar + _____ 3315P → _____ + 3215P23893Np + 0-1β → ______
  2. _____ → 18776Os + 0-1β23893Np → ______+ 0-1β
  3. 136C → ____ + 42He23692U → 9436Kr + ______+ 310n

General Chemistry Fall Final Exam Study Guide (Ch.1-6 and Ch.21)

Ch1: Matter and Change

Vocab: chemical, matter, atom, chemical change, physical change, reactant, product

Periodic Table: Groups/Families, Periods, Alkali Metals, Alkaline Earth Metals, Halogens, Noble Gases, Metals, Nonmetals, Transition Metals, Inner Transition Metals, Lanthanides, Actinides, Metalloids, Representative Elements

Mixtures: Homogenous/Solutions, Heterogeneous

Pure Substances: atoms, compounds

Conservation of Mass, Law of Definite Proportions

Ch2: Measurements and Calculations

Vocab: quantitative, qualitative, scientific method, hypothesis, theory, control, variable, accuracy, precision, percent error

Measurements: mass, volume, length, density, time, energy

Base Units: gram, liter, meter, seconds, Joules

Metric System: M, K, H, D, d, c, m, μ, n

Dimensional Analysis: metric conversions, density

Scientific Notation

Calculator Usage: exponents, parenthesis

Ch3: Atomic Structure

Vocab: neutral, isotope, atomic number, atomic mass

Theories/Scientists: Atomic Theory/Dalton, Plum Pudding Model/Cathode Ray Tube/Thomson, Gold Foil Experiment/Rutherford, Solar System Model/Bohr, Electrons Cloud Model/Quantum Mechanical Model/Shrodinger

Subatomic Particles: proton, neutron, electron

Structure: nucleus, cloud

Ch4: Electrons in Atoms

Vocab: photon, frequency, wavelength, photoelectric effect, line emission spectrum, ground state, excited state

Formulas: c = λν and E = hν

Variables: ν = frequency (Hertz = cycle/sec = 1/sec = sec -1), λ = wavelength (1m = 100cm), energy (Joules)

Constants: c = speed of light = 3.00 x 108 m/s and h = Planck’s constant = 6.626 x 10 -34 J* s

Wave/Particle Duality of Motion: photoelectric effect, line emission spectra, electromagnetic radiation (which evidence supports waves or particles)

Scientists: Planck, Heisenberg, de Broglie, Einstein, Hund, Pauli

Electron Configurations: energy levels (n), sublevels (s,p,d,f), orbitals (1,3,5,7), electrons (2,6,10,14), the Aufbau Principle, Noble Gas Notation, maximum orbitals = n2, maximum electrons = 2n2

Ch5: Periodic Trends

Vocab: ionization energy, electronegativity, electron affinity, atomic radii, ionic radii, periodic law, valence electrons, cations, anions

Scientists: Mendeleev, Moseley

Ch6: Bonding

Vocab: ionic character, octet rule, Lewis structure, ion, malleable, ductile, lustrous

Compounds and their Properties: Ionic and Molecular

Bonds: Ionic, Covalent, Metallic

VSEPR: linear, bent, trigonal planar, trigonal pyramidal, tetrahedral

Polarity: nonpolar covalent bond, polar covalent bond, nonpolar molecule, polar molecule

Intermolecular Attractions (Forces): hydrogen bonds, dipole interactions, London dispersion forces

Ch21: Nuclear Chemistry

Vocab: nuclide, nucleon, radioisotope, decay/emission, absorption/capture, fission, fusion

Nuclear Stability: proton to neutron ratio

Radiation: alpha, beta, gamma, positron, proton, neutron

Half-lives

Study all your chapter notes and vocabulary!!

  1. What is the formula for Lead (II) chromate? ______Aluminum sulfate? ______
  2. Name the compounds: Ni(ClO3)2, ______Zn3(PO4)2, ______KClO3, ______CF4,______N2_,______O4, ______SO3,______
  3. What is the formula for: nitrogen trifluoride ______, sulfur dichloride ______, nitrogen monoxide,______
  4. When is a Roman numeral used in naming a compound? ______When is a prefix used? ______
  5. What is the molar mass of KClO3?
  1. How mass in grams of 3.5 moles of KClO3?
  1. How many molecules of the KClO3 are found in 3.5 x 108 grams of KClO3?
  1. How many atoms of oxygen are in 5.05 x 102 g of KClO3 ?
  1. What is the percentage of oxygen in SO2?
  2. What is the percentage of Cu in CuCl2?
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