Module 3 Flashcards
(24 cards)
What was Rutherford’s main contribution to the study of atomic structure?
He experimentally determined that the plum pudding model of the atom was wrong and proposed his own model of the atom, which we call the planetary model. Thus became the base for Bohr’s model.
What do we call the experimental apparatus that William Crookes used in his experiments, and what did he discover with it?
Crookes tube, he used it to disc0ver cathode rays, which were later determined to be electrons.
2 electrically charged particles repel one another, what can we conclude about their charges?
they must have the same type of charge.
If a substance has 9 positive charges and 11 negative charges, is It positively charged, negatively charged, or neutral?
negatively charged
Give the location within the atom for a proton, electron, and a neutron.
protons and neutrons are tightly packed together in the nucleus of the atom. Electrons are outside of the nucleus.
Why is it so hard to separate one isotope from another?
Because isotopes behave identically in terms of chemistry, it is nearly impossible to separate them.
What were the differences between the plum pudding model of the atom and the planetary model of the atom?
the plum pudding model has positive and negative charges equally dispersed through out the entire atom. the planetary model has positive charges concentrated at the center of an atom with the negative charges whirling around them.
What is meant by saying that wavelength and frequency are inversely proportional to each other?
When one gets longer the other gets shorter and vice versa.
if you have an orange light bulb and a violet one, which emits waves with the largest wavelength? Which emits light of the higher Frequency? Which emits the higher energy light?
wavelength-orange
Frequency-violet
energy -violet
2 Light bulbs emit light of the same color. However, one is much brighter than the other, What can you say about the wavelengths and amplitudes of the waves being emitted by each bulb?
the wavelengths emitted are the same, but the brighter bulb emits a larger amplitude.
If an atom absorbs energy, what happens to its electrons? If the atom is emitting light, what are its electrons doing?
when they absorb energy the electrons jump to higher energy orbitals. When they emit light the electrons are dropping down into lower energy orbitals
What is the concept of ground state and why is it so important in chemistry?
the ground state of any substance is its lowest possible energy state. this is important because all matter strives to reach its lowest state.
The 3 fundamental particles that make up the atom are the proton, neutron, and electron. Order them in terms of decreasing mass.
neutron, proton, and electron
define and give one example of a physical constant.
a physical constant is a measurable quantity in nature that does not change.
the speed of light-c = 3.0 x 10^8 m/s
Planck’s constant-h = 6.63 x 10^-34 J/Hz
Describe what an orbital is.
It is a region of space where an electron is most likely to be found.
What is the first rule of electrical charges?
Like charges repel one another
What is the second rule of electrical charges?
Opposite charges attract each other
What is the third rule of electrical charges?
Every substance on earth has electrical charges. However, if the number of positive charges equals the negative charges, the substance is neutral with no overall charge (-1 + 1 = 0). If there is more of one charge than the other, the substance takes on that electrical charge (-2 + 1 = -1)
What is the equation for frequency?
f = c / w (w = c / f)
What is the equation for energy?
e = h x f
For 23Na, the number 23 stands for the ________.
a. number of protons and neutrons
b. mass number
c. both a and b
d. neither a nor b
c
Rutherford’s experiment showed that _______.
a. Uranium could be used for an atomic bomb
b. electrons existed as part of the atom
c. protons existed as part of the atom
d. As a light wave’s frequency increases, the wavelength decreases
e. none of the above
c
Note:
Be careful of copy errors
How many electrons do the first four electron orbitals hold?
s-2 electrons, p-6 electrons, d-10 electrons, f-14 electrons
