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Chemistry Unit 3: Atoms and the Periodic Table Flashcards | StudBud
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Chemistry Unit 3: Atoms and the Periodic Table
Chemistry Unit 3: Atoms and the Periodic Table
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#ennishighschool #chemistry
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1
If you are working with chemicals in a lab, which one of these things should you NOT do?
Keep notes on all your lab activities
Pour unused chemicals back in the original container.
Wash skin with lots of water if you touched a chemical
Be careful and take precautions will all chemicals.
2
Why did Mendeleev arrange his periodic table by atomic mass instead of atomic number?
Atomic mass is unrelated to reactivity.
Atomic number had not been discovered yet.
Different isotopes have different atomic masses.
It made neater rows.
3
What is used to calculate the average atomic mass of an element?
the isotopes that are man made
the least common isotopes
Naturally occurring isotopes
the 5 most abundant isotopes
4
How many neutrons would the atom below have?
20
18
16
32
5
Element X is 72.15% isotope type 1 (84.92 amu) and 27.85% type 2 (86.91 amu). Atomic mass?
85.13 amu
86.21 amu
86.49 amu
85.47 amu
6
Which is true of atomic radii?
Atomic radius decreases from top to bottom
Atomic radius increases from left to right
The atomic radius increases from top to bottom
atomic radius is always equal to atomic number
7
Which scientist showed electrons in specific, fixed orbits?
Quantum Model
Planck Model
Bohr Model
Rutherford Model
8
As the atomic number on the periodic table increases, the number of electrons____.
does not change
decreases
increases
alternates
9
What is the mass number of carbon isotope that has 6 protons, 6 electrons, and 7 neutrons?
12
13
2
20
10
What family represents Group 1 on the periodic table?
Alkaline Earth
Transition Metals
Alkali Metals
Noble Gases
11
Which statement describes Henry Moseley's contribution to the modern periodic table?
He predicted properties of missing elements
He arranged elements by properties
He threw out the existing table and started over.
He provided a basis for ordering the elements
12
Why is an atom considered electrically neutral?
Electrons equal the number of protons.
Neutrons equal the number of protons.
Proton forces pull on the neutrons.
Electrons equal the number of neutrons.
13
Wavelength emitted by He atoms is 656 nm. What is the frequency? (1m=10
9
nm, and c=3 x 10
8
m/s)
1.97 X 10-6 Hz
1.97 X 1014 Hz
4.57 X 1014 Hz
4.57 X 10-6 Hz
14
Which is true about Copper-60?
31 electrons
60 neutrons
29 protons
28 neutrons
15
Which statement is true regarding atoms?
Atoms contain only protons.
Chemical reactions divide atoms into smaller units.
Atoms of the same element may have different mass numbers.
Atoms usually do not combine with other atoms.
16
From which of the following atoms would it be most difficult to remove an electron?
Sodium
Sulfur
Chlorine
Aluminum
17
As a wavelength of a wave increases, what is also true?
Panck's constant will decrease
The speed of the wave will increase
The energy of the wave will increase
The frequency of the wave will decrease
18
Which describes the properties of the noble gases?
They are generally unreactive.
They are highly reactive.
They have high boiling points.
they are solid at room temperature.
19
Which statement is true comparing the research of Bohr, Rutherford, and Dalton?
Dalton and Rutherford modeled their experiments after Bohr
Rutherford and Bohr modeled their experiments after Dalton
They all had cottage cheese for breakfast.
They all developed theories at exactly the same time
20
The elements described below belong to which group/family?
Noble Gases
Alkaline Earth
Halogens
Alkali Metals
21
The number of valence electrons in Group 2 elements is.....
3
2
1
8
22
Using the periodic table, predict which elements will have similar chemical properties.
Rubidium (Rb), Yttrium (Y), and Zirconium (Zr)
Cadmium (Cd), Calcium (Ca), and Carbon (C)
Nitrogen (N), Sulfur (S), and Bromine (Br)
Magnesium (Mg), Strontium (Sr), and Barium (Ba)
23
Which law is illustrated by the example below?
law of conservation of mass
law of conservation of energy
law of definite proportions
law of indefinite proportions
