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Chemistry final 67-117 Flashcards | StudBud
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Chemistry final 67-117
Chemistry final 67-117
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1
The principal quantum number indicates what property of an electron?
Energy level
Electron cloud shape
Speed
Position
2
Why did J.J Thomson reason that electrons must be a part of the atoms of all elements ?
Cathode rays can be deflected by magnets
Cathode rays are negatively charged particles
Charge-mass ratio of electrons was the same no matter what
And electron is 2000 times lighter than a hydrogen atom
3
How is the number of neutrons in the nucleus of an atom calculated?
Subtract the # Of Electrons From The Number Of Protons
Add the number of electrons and protons together
Subtract the number of protons from the mass number
Add the mass number to the number of electrons
4
When electron moves from a lower to a higher energy level the electron...?
Always doubles it's energy
Absorbs a quantum of energy
Moves closer to the nucleus
absorbs a continuously variable amount of energy
5
If the temperature of a piece of steel decreases, what happens to its density?
The density first increases, then decreases
The density does not change
The density increases
The density decreases
6
How does the energy of an electron change when electron moves closer to the nucleus ?
It stays the same
It decreases
It doubles
It increases
7
Isotopes of the same element that have different...?
atomic numbers
Numbers of protons
Numbers of electrons
Numbers of neutrons
8
Which hypothesis led to the discovery of the proton?
A proton should be 1840 times heavier than an electron
Cathode rays are attracted to a positively charged plate
A neutral hydrogen loses one positively charged remains
The nucleus of an atom should contain neutrons
9
The range in size of most atomic radii is approximately...?
5 x 10-21 m to 2 x 10 -20 m
2 to 5 cm
5 x 10-11 m to 2 x 10 -10 m
2 to 5 nm
10
In Bohr's model of the atom where are the electrons and protons located?
Electrons occupy fixed positions around protonsin the center
They both are located throughout the atom- not free to move
They move around the protons, which are in the center
They both move throughout the Atom
11
Emission of light from an atom occurs when an electron..?
Falls to the nucleus
Drops from a higher to lower energy level
Moves within its atomic circle
Drops from a lower to a higher energy level
12
Using the periodic table, determine the number of neutrons in
16
O.
16
4
24
8
13
As changes in energy levels of an electron increase the frequencies ofan atomic line spectra...
they emit decrease
The emition cannot be determined
they emit remain the same
they emit increase
14
Which of the following sets of symbols represent isotopes of the same element?
91/42 J, 92/42 J, 93/40 J
50/19 L, 50/20 L, 50/21 L
138/59 Q, 133/55 Q, 133/54 Q
84/38 M, 86/38 M, 87/38 M
15
All atoms are...?
Neutral, protons = electrons = neutrons
Neutral, protons equals electrons
Negatively charged, more electrons than protons
Positively charged and more protons than electrons
16
Which of the following is true about subatomic particles?
Protons are positive and are the lightest particle
Electrons are negative- are the heaviest subatomic particle
The mass of a neutron nearly equal is the mass of a proton
Neutrons have no charge and are the lightest particle
17
Which of the following statements is NOT true?
Electrons are negatively charged and have a mass of 1 amu
Protons have a positive charge
The nucleus of an atom is positively charged
Neutrons are located in the nucleus of an atom
18
Which of the following is necessary to calculate the atomic mass of an element?
The masses of each isotope of the element
The atomic mass of the element
The atomic mass of carbon 12
The relative masses of the elements protons and neutrons
19
Which of the following is correct concerning subatomic particles?
The electron was discovered by Goldstein in 1886
The proton was discovered by Thompson an 1880
Cathode rays were found to be made of protons
Neutron was discovered by Chadwick in 1932
20
What is the number of electrons in the outer most energy level of an oxygen atom?
6
8
2
4
21
In which of the following is the number of neutrons correctly represented ?
75/33As has 108 neutrons
19/9 F has zero electrons
24/12 Mg has 24 neutrons
238/92 U has 146 neutrons
22
Which of the following equals one atomic mass unit ?
The mass of one helium-4 atom
The mass of one electron
The mass of one carbon-12 atom
one-twelfth the mass of one carbon-12 atom
23
What is the basis for exceptions to the Aufbau diagram?
Electron configurations are only probable
Filled and 1/2 filled are more stable than partially filled
Some elements have unusual atomic orbitals
Electron spins are important in findinelectron configuration
24
How do you high-energy models compared to lower energy levels of the atom?
They are>in magnitude than lower energy levels
There is no difference in magnitude
They are > in magnitude than the lower ener levels
No answer can be determined
25
What is the shape of the 3p atomic orbital?
Sphere
Two perpendicular dumbbells
Dumbbell
Bar
26
Which was originally a part of Dalton's atomic theory, but had to be revised about century ago?
Atoms of different elements can mix with one another
Atoms of the same element are identical
Compounds are made by combining atoms
Atoms are tiny indivisible particles
27
In which is the symbol of the element number of protons and number of electrons given correctly
F, 19 protons, 19 electrons
Zn, 30 protons, 60 electrons
In, 49 protons, 49 electrons
Cs, 55 protons, 132.9 electrons
28
The atomic number of an element is the total number of which particles in the nucleus ?
Protons
Neutrons
Protons and electrons
Electrons
29
What is the electron configuration of potassium?
1s22s22p23s23p64s1
1s22s22p63s23p63d1
1s22s22p63s23p3
1s22s22p63s23p64s1
30
As a consequence of the discovery of the nucleus by Rutherford, what model is considered true ?
Evenly distributed protons, electrons, and neutrons
The nucleus is made up of electrons and protons
Electrons occupy most of the volume of the atom
The nucleus is made of protons, electrons, and neutrons
31
What is the maximum number of f orbitals in any single energy level of an atom?
1
7
5
3
32
What is the maximum number of orbitals in the p sublevel?
3
4
2
5
33
Which type of electromagnetic radiation includes the wavelength 10
-7
m?
Gamma ray
Radio wave
Microwave
Visible light
34
If a liter of water is heated from 20°C to 50°C, what happens to its volume?
The volume increases
The volume first increases, then decreases
The volume decreases
The volume first decreases, then increases
35
Dalton said atoms are indivisible and that all atoms of an element identical. It is now known..
Atoms of an element can have different numbers of protons
Atoms are divisible
All atoms of an element are not identical but they have=mass
All of daltons hypothesis are correct
36
What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p ?
4s
3f
3d
2d
37
Why do we use relative mass of atoms compared to reference isotope rather than actual masses ?
Electron mass is way bigger compared to proton mass
Atom masses are very small and difficult to work with
The number of subatomic particle's varies
The actual masses are not known
38
Which unit is used to measure weighted average atomic mass?
Angstrom
Nanogram
Gram
Amu
39
What is the wavelength of an electromagnetic wave that travels at 3x10
8 m/s
frequency 60 MHz
300,000,000 m/s / 60,000,000 Hz
No answer can be determined
60,000,000 Hz/ 300,000,000 m/s
60 MHz x 300,000,000 m/s
40
How many unpaired electrons are in the sulfur atom ( atomic number 16 )?
1
3
0
2
41
Which of the following quantum leaps would be associated with the greatest energy of light ?
n = 2 to n= 5
n = 5 to n = 1
n = 5 to n = 4
n = 4 to n = 5
42
Isotopes of the same element have different ...?
Chemical behavior
atomic numbers
Mass numbers
Positions on the periodic table
43
The atomic mass of an element depends upon the ...?
Mass and relative abundance of each isotope of that element
Mass of each isotope of that element
Mass of each electron in that element
Relative abundance of protons in that element
44
What is the maximum number of electrons in the second principal energy level?
2
32
18
8
45
If the spin of one in an orbital is clockwise, what is the spin of another in that orbital ?
Both clockwise and counterclockwise
Zero
Counterclockwise
Clockwise
46
What is the approximate frequency of a photon having an energy 5x10
-24
J? (h=6.6x10
-34
J*s)
1 x 10-10 Hz
3 x 10-57 Hz
3 x 10-58 Hz
8 x 109 Hz
47
Stable electron configuration's are likely to contain...?
Unfilled S orbitals
Fewer electrons than unstable configurations
Electrons with a clockwise spin
Filled energy sub levels
48
How do the isotopes of hydrogen-1 and hydrogen-2 differ?
Hydrogen-2 has one neutron; hydrogen-1 has none
Hydrogen-2 has one proton; hydrogen-1 has none
Hydrogen-2 has two protons; hydrogen-1 has one
Hydrogen-2 has one more electron than hydrogen-1
49
Which of the following electromagnetic waves have the highest frequencies ?
Microwaves
X-rays
Gamma rays
Ultraviolet light waves
50
Dalton's atomic theory included which idea ?
Individual atoms can be seen with a microscope
Atoms of the same element are always identical
All atoms of elements are of the same size
Atoms of different elements always combine in a 1:1 ratio
