Download std 1 sem review 1011wanswers

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Date:________________ Period:_____
The periodic table displays the elements in increasing atomic number and shows how
periodicity of the physical and chemical properties of the elements relates to atomic structure.
As a basis for understanding this concept:
1a: Students know how to relate the position of an element in the periodic table to its atomic
number and atomic mass.
1. Which of the following ordered pairs of
elements shows an increase in atomic
number but a decrease in average
atomic mass?
A Ag to Pd.
B Co to Ni.
C Ge to Sn
D Cr to Mo .
2. Why is colbalt (Co) placed before nickel (Ni) on the periodic table of elements even
though it has a higher average atomic mass than nickel?
A Nickel has one more proton
B Cobalt was discovered first
C Nickel has fewer electrons
D Cobalt has a lower density
3. Generally, how do atomic masses vary throughout the periodic table?
A they increase from left to right and top to bottom
B they increase from left to right and bottom to top
C they increase from right to left and top to bottom
D they increase from right to left and bottom to top
4. Iodine would have chemical properties
most like:
A manganese (Mn)
B tellurium (Te)
C chlorine (Cl)
D xenon (Xe)
27
5. How many protons are in ? 13
A 13
B. 14
C. 3
Al
D 27
1b: Students know how to use the periodic table to identify metals, semimetals, nonmetals,
and halogens.
6. Which of the following would be classified as a metal?
A bromine (Br)
B helium (He)
C sulfur (S)
D lithium (Li)
7. Which type of element is the most abundant in the periodic table?
A non-metals
B semi-metals
C metals
D metalloids
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1c: Students know how to use the periodic table to identify alkali metals, alkaline earth metals
and transition metals, trends in ionization energy, electronegativity, and the relative sizes of
ions and atoms.
8. The chart above shows the relationship
between the first ionization energy and
the increase in atomic number. The letter
on the chart for the alkali family of
elements is:
A W
B X
C Y
D Z
9. Which of the following atoms has the
largest atomic radius?
A barium (Ba)
B chorine (Cl)
C iodine (I)
D magnesium (Mg)
For questions 10-14, match the group name with its description.
10. Alkali Metals e
a. group that will take on a +1 to a +3 charge
11. Alkali Earth Metals b
b. group that will have a valence configuration of s2
12. Halogens c
c. very reactive non-metals
13. Noble Gases d
d. non-reactive gases
14. Transition Metals a
e. the group that has the largest atomic radii
1d: Students know how to use the periodic table to determine the number of electrons
available for bonding.
15. Which of the following atoms has six valence electrons?
A magnesium (Mg)
B silicon (Si)
C sulfur (S)
D argon (Ar)
16. Which of the following has no electrons available for bonding?
A magnesium (Mg)
B silicon (Si)
C sulfur (S)
D argon (Ar)
17. Which of the following has 4 electrons available for bonding?
A magnesium (Mg)
B silicon (Si)
C sulfur (S)
D argon (Ar)
18. An unknown elements’ electron configuration is: 1s22s22p63s23p64s23d104p65s1. what
element is it?
A potassium (K)
B rubidium (Rb)
C gallium (Ga)
D indium (In)
19. What is the valence electron configuration for Selenium (Se)?
A 3s23p6
B 3s23p4
C 4s23d104p4
D 4s23d104p6
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1e: Students know the nucleus of the atom is much smaller than the atom yet contains most
of its mass.
20. Which statement best describes the density of an atom’s nucleus?
A The nucleus occupies most of the atom’s volume but very little of its mass.
B The nucleus occupies very little of the atom’s volume and contains little of its mass.
C The nucleus occupies most of the atom’s volume and contains most of its mass.
D The nucleus occupies very little of the atom’s volume but contains most of its mass.
*1h: Students know the experimental basis for Thomson's discovery of the electron,
Rutherford's nuclear atom, Millikan's oil drop experiment, and Einstein's explanation of the
photoelectric effect.
21. What information do the experimental
results above reveal about the nucleus of
gold?
A The nucleus contains less than half of the
mass of the atom.
B The nucleus is small and is the densest
part of the atom.
C The nucleus contains small positive and
negative particles.
D The nucleus is large and occupies most of
the atom’s space.
1j* Students know that spectral lines are the result of transitions of electrons between energy
levels and that these lines correspond to photons with a frequency related to the energy
spacing between levels by using Planck's relationship (E = hv).
22. When a metal is heated in a flame, the flame has a distinctive color. This information
was eventually extended to the study of stars because:
A the color spectra of stars indicate which elements are present.
B a red shift in star color indicates stars are moving away.
C star color indicates absolute distance
D it allows the observer to determine the size of stars.
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