Measurement
Atomic Structure
Isotopes
Periodic Table
Periodic Trends
100
The SI (metric) base unit for length
Meter
100
The three parts of an atom.
Proton, neutron, and electron
100
Changing these subatomic particles in an atom create different isotopes
Neutrons.
100
Mendeleev arranged his table by increasing atomic mass, but today we arrange it by this.
Atomic number
100
The number of valence electrons in an atom increases as you move this direction on the periodic table.
Left to right.
200
The unit that is larger than a liter by a factor of 3.
Kiloliter
200
The subatomic particles that are inside the nucleus.
Protons and neutrons.
200
This subatomic particle is the same for all isotopes of an element
Protons
200
These elements, found between metals and nonmetals, share properties of both.
Metalloids
200
Atomic radius gets larger when you move this direction in a group on the periodic table.
Down
300
The equivalent to 987 mm in meters.
0.987 meters
300
The only part of the atom that does not contribute to its mass.
Electron
300
The mass number of this oxygen isotope.
16.
300
The vertical columns on the periodic table are called this.
Groups
300
As you move left to right across the periodic table, ionization energy generally does this.
Increases
400
476000000 in scientific notation
4.76 x 10^8
400
In order to create a neutral atom, these two subatomic particles must be equal in value.
Protons and Electrons
400
The isotope of carbon with 8 neutrons.
Carbon-14
400
All elements in the same group have this in common.
Number of valence electrons.
400
These elements in Group 18 usually don’t have electronegativity values because they do not chemically bond.
Noble Gases
500
The wavelength of red light is about 6.5 × 10⁻⁷ meters. Express this in nanometers (nm) (10-9 m).
650 nm
500
An atom has 17 protons, 18 neutrons, and 17 electrons. Identify the element and its charge.
Chlorine; neutral
500
An atom has 15 protons, 16 neutrons, and 15 electrons. Write the isotope’s name and symbol in standard notation.
Phosphorous-31
500
Although both belong to Group 1, hydrogen is often placed separately from the alkali metals. Explain why this is.
It does not share the same metallic properties with the other alkali metals in this group.
500
Explain why atomic radius increases down a group, but decreases across a period.
As you add electron shells down a group, the radius gets larger; as you add an electron to the shell across a period, they are pulled in more by added protons.