CHEMISTRY 1ST SEMESTER EXAM REVIEW

1. A measure of the quantity of matter is 2. List a process that is a physical change. 3. List a process that is a chemical change? 4. A chemical change occurs when

5. A physical change occurs when a

MASS

CUTTING, GRINDING, TEARING

BURNING

MOLECULES ARE REARRANGED TO FORM A NEW COMPOUND

MOLECULES ARE MOVED AROUND, BUT ARE STILL MADE OF THE SAME COMPONENTS

6. A state of matter in which a material has no definite shape but has a definite volume is the ____ state. 7. Under ordinary conditions of temperature and pressure, the particles in a gas are 8. The liquid state of matter can be described as

9. A solid substance is

LIQUID

RANDOMLY SPREAD FAR APART

HAVING A DEFINED VOLUME BUT NO DEFINED SHAPE

STATE OF MATTER WITH A DEFINED SHAPE AND DEFINED VOLUME

10. If a mixture is uniform in composition, it is said to be 11. If a mixture is not uniform throughout, it is called 12. The quantity of matter per unit volume is 13. The relationship/equation between the mass m of a material, its volume V, and its density D is 14. The density of aluminum is 2.70 g/cm3. What is the mass of a solid piece of aluminum with a volume of 1.50 cm3?

HOMOGENEOUS

HETEROGENEOUS

DENSITY

D = M/V

4.05 G

15. A sample of gold has a mass of 96.5 g and a volume of 5.00 cm3. The density of gold is 16. The density of pure diamond is 3.5 g/cm3. What is the volume of a diamond with a mass of 0.25 g? 17. How many significant figures are in 0.202grams? 18. How many significant figures does 30.00 have?

19.3 G/CM3

.07 CM3

THREE

FOUR

19. The speed of light is 300 000 km/s. Rewrite this in scientific notation. 20. The average distance between the Earth and the moon is 386 000 km. Rewrite this in scientific notation. 21. In oxides of nitrogen, such as N2O, NO, NO2, and N2O3, atoms combine in small whole-number ratios. this evidence supports the law of

22. If two or more compounds are composed of the same two elements, the ratio of the masses of one element that combines with a fixed mass of the other element is a simple whole number. This is a statement of the law of

3.0 X 105

3.86 X 105

MULTIPLE PROPORTIONS

MULTIPLE PROPORTIONS

23. Oxygen can combine with carbon to form two compounds, carbon monoxide and carbon dioxide. The ratio of the masses of oxygen that combine with a given mass of carbon is 1:2 This is an example of:

24. According to the law of definite proportions, any two samples of KCl have

25. According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a compound, the mass of the compound is _____ the sum of the masses of the individual elements.

26. An atom is electrically neutral because:

MULTIPLE PROPORTIONS

EQUAL/DEFINED PROPORTIONS OF K TO Cl

THE SAME AS

IT HAS EQUAL PROTONS(+) AND ELECTRONS (-)

27. The number of atoms in one mole of carbon is

28. Avogadro’s number represents what amount? 29. How many moles are in 15 grams of Lithium?

30. How many grams are in 3.3 moles of Potassium Sulfide, K2S?

31. How many molecules are in 52 grams of CO?

32. What is the mass of 3.01x1023 molecules of Fe2O3?

6.022 x 1023

The number of molecules in a mole

2.16 moles

363.86 grams

1.12 x 1024

79.8 grams

33.The statement that an electron occupies the lowest available energy orbital is what law/principle?

34.“Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and all electrons in a singly occupied orbital must have the same spin” is a statement of what law/principle?

35.The statement that no two electrons in the same atom can have the same four quantum numbers is what law/principle?

36.Which rule requires that each of the P orbitals at a particular energy level receive one electron before any of them can have two electrons?

THE AUFBAU PRINCIPLE

HUND’S RULE

PAULI’S EXCLUSION PRINCIPLE

HUND’S RULE

37. The sequence in which energy levels are filled is specified by what law/principle?

38. The Aufbau Principle states that an electron

39. The Pauli Exclusion Principle states that no two electrons in the same atom can

40. What is the correct order of atomic orbitals filled according to the Aufbau Principle?

THE AUFBAU PRINCIPLE

FILLS UP THE LOWEST ENERGY LEVEL FIRST, THEN BUILDS UP

HAVE THE SAME SET OF QUANTUM NUMBERS, & CAN’T BE IN THE SAME PLACE AT SAME TIME

1S, 2S, 2P, 3S, 3P, 4S, 3D, 4P

41.The element with electron configuration 1s22s22p63s23p2 is

42.The electron configuration for the Carbon atom, C, is 1s22s22p2. The atomic number of Carbon is

43.What is the electron configuration for Nitrogen, N atomic number 7?

44.The electron configuration for Aluminum, Al, atomic number 13 is

45. Write the correct electron configuration for Fluorine:

46. Which element has the following electron configuration: 1s22s22p63s23p64s23d8?

Which element has the following electron configuration: [Ne]3s1?

SILICON, Si

6

1S22S22P3

1S22S22P63S23P1

1s22s22p5

NICKEL, Ni

47. Which element has the following electron configuration: [Ne]3s1?

48. The higher the frequency of a wave, the ________ the energy of that wave.

49. The higher the wavelength of a wave, the __________ the energy of the wave.

50. This individual is responsible for the organization of one of the first periodic tables which was organized based on the atomic mass of the known elements.

51. This individual is responsible for organization of the present day periodic table which is based on the increasing number of protons in the nucleus.

SODIUM, Na

HIGHER

LOWER

DIMITRI MENDELEEV

HENRY MOSELEY

52.What is the group of radioactive elements called with the atomic numbers from 90 to 103?

53.The elements with atomic numbers from 58 to 71 are called?

54. Argon, Krypton, and Xenon are all examples of what group of elements?

55. The periodic law states that

56. Elements in a group or column in the periodic table can be expected to have similar

ACTINIDES

LANTHANIDES

NOBLE GASES

THE PHYSICAL AND CHEMICAL PROPERTIES OF THE ELEMENTS ARE FUNCTIONS OF THEIR ATOMIC NUMBERS

PROPERTIES

57. The elements in Group 1 are also known as the

58. The most reactive group of nonmetals are the

59. The soft, silvery, reactive metals, all of which have one electron in its s orbital is known as the

60. The most characteristic property of the noble gases is that they are

ALKALI METALS

HALOGENS

ALKALI METALS

UNREACTIVE

61.A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called

62.When an electron is acquired by a neutral atom, the energy is called

63.As you move down a group of elements you expect to see the atomic radii

64. Across a period in the period table, ionic radii

65. Groups 1-2 and 13-18 are known as this

ELECTRONEGATIVITY

ELECTRON AFFINITY

INCREASE

DECREASES

MAIN GROUP ELEMENTS

66.What is the correct block, period and group for the element with the electron configuration [Kr]5s2 ?

67. What are the 2 main types of bonds that we have learned about so far?

68.During an ionic bond, valence electrons are____ 69. During a covalent bond, valence electrons are_____ 70.What periodic trend can be used to determine the type of bond that elements will form?

BLOCK: S PERIOD: 5 GROUP: 2

COVALENT AND IONIC

TAKEN OR GIVEN AWAY

SHARED

ELECTRONEGATIVITY

71. When using the electronegativity difference method, what amounts correspond to what bonds?

72. If Sodium, Na, was to bond with Chlorine, Cl, what type of bond would they form?

73. If Bromine, Br was to bond with Chlorine, Cl, what type of bond would they form?

74. If Hydrogen, H was to bond with Oxygen, O, what type of bond would they form?

Nonpolar Covalent: 0.0-0.3, Polar Covalent: 0.3-1.7, Ionic: 1.7-4.0

IONIC

NONPOLAR COVALENT

POLAR COVALENT

STUDY HARD, AND AS ALWAYS, MAY THE ODDS BE EVER IN YOUR

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