Download Chapter 6 Review“The Periodic Table”

Review“The Periodic Table”
1. How is the number of neutrons in the nucleus of an atom calculated?
Mass – atomic number
2. All atoms are neutral, with the number of protons equaling the ___.
# electrons
3. Isotopes of the same element have different _____. # neutrons
4. Using the periodic table, determine the number of neutrons in 16O.
16- 8 = 8 neutrons
5. What does the number 84 represent in the name krypton-84? mass
6. What is the correct complete symbol for an atom of tritium? 31H
mass
at # Symbol
7. Dalton said that atoms were indivisible and atoms of the same
element were identical. Have any changes been made to this? Yes –
isotopes have different number of neutrons
8. The mass number of an element is equal to _____. Number protons +
neutrons
9. The sum of the protons and neutrons in an atom equals the __.
Atomic mass
10.
The atomic number of an element is the total number of ____.
Number protons
11.
How do the isotopes of hydrogen-1 and hydrogen-2 differ?
neutrons
12.
A fictitious element “X” has 10.0 % of the isotope with mass 55
amu, 20.0 % of the isotope with mass 56 amu, and 70.0 % of the
isotope with mass 57 amu. Estimate the atomic mass of element X.
(.10 x 55) + (.20 x 56) + (.70 x 57) = 56.6 amu
13.
Element “Z” has two isotopes: one has mass number of 19.0
amu is 55.0 % abundant, and the isotope with mass number 21.0 amu
is 45.0 % abundant. What is the average atomic mass for element Z?
(.55 x 19) + (.45 x 21) = 19.9 amu
14.
How many protons are present in an atom of Beryllium-9? 4
(atomic number)
15.
Calculate the number of neutrons in Lead-210. 210-82 = 128
neutrons
16.
Determine the number of electrons in an atom of Iridium. 77 e-
17.
About how many more times massive is a proton than electron?
1840 times
18.
How many neutrons are present in an isotope of uranium-235?
235 – 92 = 143 neutrons
19.
What is the atomic number for an element with 41 neutrons and
a mass number of 80? 80 - 41 = 39
20.
What is the maximum number of electrons in the second
principal energy level? 2s2 2p6 = 8
21.
If three electrons are available to fill three empty 2p atomic
orbitals, how will the electrons be distributed? ↑ ↑ ↑
22.
What is the maximum number of electrons in the second
principal energy level? REPEAT
23.
If three electrons are available to fill three empty 2p atomic
orbitals, how will the electrons be distributed? REPEAT
24.
What types of atomic orbitals (s, p, d, or f) are in the third
principal energy level? S, P, D
3rd row = 3s23p63d10
25.
How would the atomic emission spectra of a sodium atom on
Earth compare with sodium in the sun?
Would be the same
26.
How many energy sublevels are in the second principal energy
level? S, P (2nd row = 2s22p6)
27.
Emission of light from an atom occurs when an electron _____.
Releases energy and returns to ground state
28.
Which of the following elements has the smallest radius: a)
chlorine, or b) bromine?
29.
The modern periodic table is arranged according to _____.
Atomic number (protons)
30.
Which of the following elements are nonmetal: Pt, V, Li, and
Kr
31.
or
Which of the following elements is a transition metal: a) copper,
b) cesium?
32.
What is the factor that contributes to the increase in ionization
energy from left to right across a period?
Smaller size = stronger hold on electrons
33.
To what category of elements does an element belong if it is a
poor conductor of electricity?
nonmetals
34.
Which of these elements has the lowest electronegativity value:
a) cesium, or b) calcium?
Left or Lower = Larger = lower electronegativity value
35.
Which of the following is correct: a) In, 49 protons, 49
electrons or b) Zn, 30 protons, 60 electrons?
36.
What element in the second period has the largest atomic radius?
Lithium
37.
Which of the following elements is in the same period as
phosphorus: a) magnesium, or b) nitrogen?
38.
Who arranged the elements according to atomic mass, and used
the arrangement to predict the properties of missing elements?
Mendeleev
39.
What is true about the electron configurations of the noble
gases? Full outer shells (valance electrons)
40.
What is the element with the highest electronegativity value: a)
calcium, or b) fluorine? F is smaller
41.
Which subatomic particle plays the greatest part in determining
the properties of an element? Electrons
42.
What element has the electron configuration of 1s22s22p63s23p2?
Silicon
43.
How does atomic radius change from left to right across a period
in the periodic table? Smaller because more opposite charges
44.
How does atomic radius change from top to bottom in a group in
the periodic table? Larger because more orbitals
45.
Elements that are characterized by the filling of p orbitals are
classified as _____. Alkaline Earth metals
46.
As you move from left to right across the second period of the
periodic table, ionization energy __. Increases because smaller size
47.
Atomic size generally decreases as you ____. Move to the right
or up
48.
Each period in the periodic table corresponds to ____. Orbitals
or energy levels
49.
Compared with the electronegativity of elements on the left side
of a period, the electronegativity of the elements on the right side of
the same period tend to be ____. Higher because smaller
50.
How many electrons are there in the highest occupied energy
level of atoms in Group 5A elements? np3