Download 19. Define the law of multiple proportions. Elements form

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19. Define the law of multiple proportions.
Elements form compounds in simple whole number ratios
20. What do isotopes of the same element have in common and what is different?
Isotopes have the same number of protons, electrons and atomic number
Isotopes have a different mass number and number of neutrons
21. Explain how Rutherford’s gold foil experiment worked and what it proved.
Rutherford shot particles through gold foil. Most went through, but some bounced back. He concluded
that atoms are mostly empty space and the particles bounced off the dense center called the nucleus.
22. What subatomic particle determines the identity of an atom? Protons
23. How do you find the following:
A. Number of protons in an atom = __same as the atomic number__
B. Number of neutrons in an atom = __mass # - atomic #__
C. Number of electrons in an atom = __same as the atomic number__
Symbol
Atomic
Number
Mass Number Number of
Protons
Number of
Electrons
Number of
Neutrons
Ag
47
109
47
47
62
Mg
12
24
12
12
12
Ga
31
72
31
31
41
The Periodic Table & Trends:
24. The horizontal rows found on the periodic table are called __periods__, while the vertical columns are
called ___groups__ or ___periods___.
25. The most reactive elements on the periodic table are in group __1A – Alkali Metals__.
26. Electronegativity ____decreases_____ (increases/decreases) going down groups and
______increases_____ (increases/decreases) going across periods from left to right.
27. Ionization Energy ______decreases_____ (increases/decreases) going down groups and
______increases_______ (increases/decreases) going across periods from left to right.
28. Atomic radius ________increases______ (increases/decreases) going down groups and
_______decreases_______ (increases/decreases) going across periods from left to right.
29. The number of valence electrons ________increases______ as you go across a period, but will
______stay the same____ as you go down a group.
30. The most electronegative element is ________Fluorine_____________.
31. The element with the largest atomic radius is _______Francium______.
32. Which of the following has a bigger atomic radius: Cesium or Calcium? (Circle one.)
33. Which of the following has a higher ionization energy: Potassium or Sulfur? (Circle one.)
34. Classify the following as either an: Alkali Metal, Alkaline Earth Metal, Halogen or Noble Gas
A.
Strontium
__Alkaline Earth Metal____
C.
B.
Bromine
___Halogen___
D. Krypton
Potassium
__Alkali Metal___
__Noble Gas____
Electron Configurations & EMR Calculations:
36. Write the long-hand electron configurations AND noble gas notations for the following atoms:
A. Calcium 1s22s22p63s23p64s2
[Ar]4s2
B. Iron 1s22s22p63s23p64s23d6
[Ar]4s23d6
37. What do the superscripts add up to in an electron configuration? ____the atomic number___
38. What is the energy of a photon whose frequency is 6.9 x 1014 Hz?
E=hxV
E = 6.63 x 10-34 x 6.9 x 1014
E = 4.57 x 10-19 J
E=hxv
h = 6.63x10-34 J·s
39. What is the packet of light called that is released when an electron relaxes to the ground state?
photon
Bonding & Ionic Compounds:
40. Name the following compounds:
A. BaCO3
_____barium carbonate____
B. NH4OH
_____ammonium hydroxide_____
C. NiCl2
_____nickel (II) chloride_____
D. MnCl3
_____manganese (III) chloride____
41. Write the formula for each of the following compounds:
A. Aluminum phosphate
______AlPO4____
B. Copper (III) sulfide
_____Cu2S3_____
C. Magnesium chloride
_____MgCl2____
D. Potassium nitrate
______KNO3____
42. Identify each of the following as either an: ionic or covalent bond
A. electrons are shared
__________covalent_______
B. electrons are transferred
_________ionic_________
C. MgCl2
________ionic_______
D. CO2
_________covalent__________
43. Why are metals malleable and ductile? _________metals have a “sea of electrons”______