THIS REVIEW SHEET IS DUE MONDAY 12/17. No exceptions!
1. Anything that takes up space and has mass ________________
2. Examples of NON matter would include any form of _____________; examples
____________________________________
3. Intensive properties are ________________________________________________________
4. Extensive properties are ________________________________________________________
5. Refers to how close a series of measurements are to one another ________________
6. Refers to how close a series of measurements are to the accepted value ________________
7. SI base unit of temperature ______; length __________; mass ________; density ________;
8. Round 42.156 cm. to four significant figures. ________ four significant figures. ________ two ______
9. Which of the following statements indicates a physical property of an element? forms new substances when … reacts with … conducts electricity … is shiny …
10. A form of matter with a definite shape and volume ________________
11. States that mass is neither created nor destroyed in any process
________________________________
12. Which of the following are compounds? calcium; sodium; calcium carbonate; phosphorous; magnesium oxide
13. The smallest particle of an element that retains the properties of that element ________________
14. ________________ theory states that all matter is composed of atoms.
15. Which subatomic particles are found in an atom’s nucleus? ________________
16. ________________ decay is a process (not requiring energy) by which unstable nuclei lose energy.
17. The set of frequencies of the electromagnetic waves emitted by the atoms of an element: atomic
___________ spectrum.
18. A particle of electromagnetic radiation with no mass that carries a quantum of energy
________________
19. The minimum amount of energy that can be lost or gained by an atom ________________
20. The lowest allowable energy state of an atom ________________
21. How many valence electrons does the group 1 elements have? ______
Group 2? ________ Group 13 ______ Group 14______Group 15______Group 16 ______ Group
17______Group 18______
22. What is the correct electron-dot structure for sodium?___________; magnesium __________ chlorine _________
23. Statement that when the elements are arranged by increasing atomic number, there is a periodic repetition of their chemical and physical properties ________________
24. A column in the periodic table is called a ________________; a row is called a _____________.
25. Elements in the same group have the same number of ________________
26. Which energy level of the period 4 transition elements is being filled with electrons?
________________
27. In which of the following pairs is the second particle listed larger than the first?
Metal atom : metal ion nonmetal atom : nonmetal ion
28. How many electrons does an atom generally need in its outer level to be the most stable?
________________
29. Diagram the electron configuration which represents the most chemically stable atom in the 3rd period, starting with the 1s sublevel.
30. Atom that has a positive or negative charge_____
Covalently bonded group of atoms that has an overall positive or negative charge
___________________ _____
31. Energy required to remove an electron from a gaseous atom: ________________ energy.
32. Statement that atoms tend to gain, lose, or share electrons to acquire a full set of eight valence electrons: __________ rule.
33. Alkaline earth metals form ions with a charge of _________. Alkali metals form ions with a charge of
______.

34. A positively charged ion: ________________. A negatively charged ion: __________________.
35. An ionic compound whose aqueous solution conducts electricity ________________
36. The electrostatic force that holds oppositely charged particles together: ________________ bond.
37. What is the formula of magnesium phosphate, which is made up of the ions Mg2+ and P043-?
________________
38. Shows the simplest ratio of ions in an ionic compound, and whose charge is neutral
________________ ________________
39. What are 5 typical properties of metals?
________________________________________________________________
What are 4 typical properties of nonmetals?
________________________________________________________________
40. According to the octet rule, most atoms that bond achieve the electron configuration of a
__________ ____.
41. In the formation of a covalent bond electrons are ________________. In the formation of an ionic bond, electrons are
________________.
42. What elements normally exists in the form of diatomic molecules?
________________________________________________
43. How many pi bonds are there in a double bond? __________; in a triple bond? ________________
Electrons are shared unequally in a ___________ covalent bond, like the bond between H and O.
44. A starting substance in a chemical reaction is called a _______________, and the ending substances are called _______________.
45. The “electron sea model” accounts for most properties of these elements: ____________.
46. A solution in which the solvent is water: an ____________ solution.
47. What is the correct formula for sodium oxide? ____________ calcium hydroxide ____________ magnesium sulfide____________ sodium sulfate ____________ nitrogen dioxide ____________ lithium bromide ____________ chlorine
____________
48) Circle the formulas which represents an ionic compound.
H2O(l) NH3(g) CCl4(L) NaCl(s) CaBr2 AgNO3 AlO3 SO2
49) List the atomic numbers of the alkali metals
________________________________________________
50) A substance that is composed only of atoms having the same atomic number is classified as a/n
__________.
51) The atomic number of an atom is always equal to the total number of ____________
52) Which atom has the largest atomic radius? A)Mg B)Na C)K D)Ca
53) The nucleus of an atom consists of 5 protons and 6 neutrons. The total number of electrons present in a neutral atom of this element is ____________
54) What is the correct chemical formula for iron (III) oxide? ____________ Iron (II) oxide ____________
55) Which element contains exactly 15 protons?
56) Which molecules are nonpolar? H2 H2O NaBr CO2
57) Which compound above contains an alkali metal and a halogen?
58) Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium atom is smaller.
The smaller radius is primarily a result of the magnesium atom having
____________________________________
59) What type of bond is formed when two non-metal atoms combine? ________________________
60) The total number of orbitals in a d sublevel is ____________
61) What particle has a mass of approximately one atomic mass unit and a unit positive charge?
____________
62) Different isotopes of the same element must have a different number of ____________ and the same _____ _______
63) Why is NH3 classified as a polar molecule?
____________________________________________________________

64) An atom of an element contains 20 protons, 20 neutrons, and 20 electrons. This element belongs to what group (name) of elements? ________________________
65) Given an atom with the electron configuration 1s22s22p3, how many orbitals are completely filled?
_______ In 1s22s22p5? _______
66) In an experiment, alpha particles were used to bombard gold foil. As a result of this experiment, the conclusion was made that the nucleus of an atom is____________ than the atom and ____________ charged.
67) A sodium atom and a sodium ion must have the same number of ____________
68) When sodium reacts with chlorine to form sodium chloride, electrons are lost by which element?
____________
69) Compared to an atom of C-12, an atom of C-14 has more of these subatomic particles:
____________
70) Which formula represents a tetrahedral molecule? H2O(l) NH3(g) CCl4(L) NaCl(s) CaBr2
71) An atom in the ground state contains 8 valence electrons. This atom is classified as a _______
________
72) What kind of particle, when passed through an electric field, would be attracted to the negative electrode? to the positive electrode? To neither electrode? alpha particle beta particle gamma ray
73) The pair of elements with the most similar chemical properties would be found in the same
____________ on the periodic table.
74) What is the electron-dot symbol for an atom with an electron configuration of 1s22s22p3?
_________ 1s22s22p4_________
75) What is an example of a homogeneous mixture? ____________ heterogeneous? ____________
76) When a sodium atom becomes an ion, the size of the atom _________ by _________ing an electron.
77) An atomic mass unit is defined as exactly _________ the mass of a _________ atom.
78) Atoms of nonmetals generally react with atoms of metals by _________ electrons to form
_________ compounds.
79) A particle of matter contains 8 protons, 9 neutrons, and 8 electrons. This particle must be a
_________ charged _________ atom.
80) What is the orbital notation that correctly represents the outermost principal energy level of a nitrogen atom in the ground state?
81) Which sublevel contains the greatest number of orbitals? s, p, d, f
82) The ozone layer is important to living organisms in that it:
_______________________________________
83) When the electrons of an excited atom fall back to lower levels, there is an emission of energy that produces ____________ lines.
84) Which of the following is/are chemical properties? Solid combustible low melting point combines with oxygen
85) What particle has a negative charge and a mass that is approximately 1/1800 the mass of a proton?
____________
86) Put the following sublevels in order from low to high energy? 4s 4p 3p 3s 5s 4d 3d
87) A water molecule is best described as polar/nonpolar with ____________ covalent bonds.
88) Combustion of methane is best described as an endothermic/exothermic physical/chemical change.
89) Which atom has the smallest atomic radius? Li F K B Ca
90) What principal energy levels has no f sublevel? ____________
91) What is the electron configuration of a fluoride ion (F-) in the ground state?
________________________
92) How many protons are in the nucleus of an atom of beryllium? ____________ carbon ____________ zinc ____________
93) List indications that a chemical change has occurred.
94) Intensive physical properties include:

95) How would you separate these mixtures? Sand and sugar __________________ Two colorless liquids ______________ coffee grounds and water ________________ sand and saltwater ______________ iron filings and sand
______________
96) Sterling silver, brass, bronze, and steel are all examples of _________________, which exhibit properties of ___________.
97) Groups 1,2, 13 - 18 on the periodic table are also known as the ____________________ elements, while groups 3 - 12 are known as
_____________________ elements, or _____________________ ______________.
98) How does the electron configuration for a group 13 element end? __________, a group 15 element
_________, group 17 ____
99) Using arrows, and the periodic table as a reference, diagram the trend for increasing: atomic radii electron affinity electronegativity
100) What are the characteristics of alkali metals?
101) A homogeneous mixture with properties of metals: __________________________
102) Strong covalent bonds have ___________ bond length and _____________ dissociation energy.
103) The smallest unit of a covalently bonded substance is called a _________________.
104. You calculate that 425 000 m is the answer to a problem. Write your answer in scientific notation.
________________
105. What are the characteristics of a compound. (see p71)
106.What type of bond exists between the carbon atoms in diamonds?
107.Which has more electrons Mg 2+ or Mg 0 ; O 2- or O 0
108.Al becomes an ion by ______ electrons. The Al ion is ______ than the Al atom. The Al ion has _____ electrons than the Al atom.
109.A _________________ covalent bond shares electron unequally.
110.Which element is in Group 3 and Period 5 of the Periodic Table?
111.An atom of which element in the ground state has a complete outermost shell (energy level)?
112.The element with _____________ electronegativity will be the negative part of a compound.
113.What two particles account for most of the mass in the atom?
114.How many valence electrons in Be ______ Al ______ Rn ______
115.The chemical properties of an atom are determined by the number of _____________________
116. Four valence electrons of an atom in the ground state would occupy what sublevels? _________
117. In the modern Periodic Table, the elements are arranged according to ____________________
118.Which particles may be gained, lost, or shared by an atom when it forms a chemical bond?
119. What type of substance can be decomposed by a chemical change?
120.To what family do the following belong: Br ______, Strontium ______________, Iodine _______,
Lithium _______, argon________
121.A oxygen ion (O 2-) has the same electron configuration as_______
122.As a fluorine atom gains electrons, its radius ______
123.A region of most probable electron location in an atom is called ___
124.Arrange the following from smallest to largest mass: proton, electron, neutron, alpha particle
125. Which molecule contains a polar covalent bond? an ionic bond? H2O NaCl CH4
126.An atom of sulfur and oxygen have the same
127.In the early 1900’s, it was proposed that energy may be absorbed or released from atoms in small, indivisible packets named ________
128.What type of bonds are formed when two non-metal atoms combine? a metal and a nonmetal? two metals?