3.6 - 3.8: Atomic Structure Electron Arrangement
Potassium has ________ valence electron(s).
1
An electron of an atom is said to be in the excited state if both the following conditions are fulfilled:
The number of electrons in any energy level is less than the maximum that can be accommodated (except the outermost shell). There are electrons in a higher energy level, leaving a lower energy level unfilled.
Write the main-shell electron configuration for neutral sulfur that has atomic number 16. Express your answer as the symbol for the element followed by the numbers of electrons in each shell, separated by commas. For example, Na 2, 8, 1. READ QUESTION CAREFULLY ?
The main-shell configuration for sulfur is S 2,8,6
The electron configuration for oxygen is 1s2s22s2s23s2s2. True False
False
Classify the following atoms as having only ground-state electrons, where all electrons occupy the lowest possible energy levels, or as having at least one excited-state electron in a higher energy level. Drag the appropriate items to their respective bins.
Ground state Phosphorus Neon Excited state Boron Nitrogen
Arrange the elements in decreasing order of the number of valence electrons. Rank from most to least number of valence electrons. To rank items as equivalent, overlap them. I S Sr Br Ca Ga Na Mg Xe F Ge Bi K Kr Sb
MOST Xe Kr I Br F S Bi Sb Ge Ga Sr Ca Mg Na K LEAST
The element with the ground state electron configuration of 1s2 2s2 2p6 3s2 is Mg. Ne. Ca. Mn.
Mg
If both the first and second shells of an atom are full, what is the total number of electrons present in that atom? Express your answer as an integer.
10
A d sublevel can hold a maximum of 10 electrons. 2 electrons. 14 electrons. 6 electrons. STUDY
10 electrons.
What is the maximum number of electrons that can occupy the 4f sublevel? 14 28 10 7 STUDY
14
The ground state electron configuration for sodium is 1s2 2s2 2p6 3s2 3p6 4s1. 1s2 2s2 2p6 3s2 3p4. 1s2 2s2 2p6. 1s2 2s2 2p6 3s1.
1s2 2s2 2p6 3s1.
Calcium has ________ valence electron(s).
2
What is the maximum number of electrons that can occupy a single d orbital? 18 8 10 2 READ QUESTION CAREFULLY
2
Which orbital will have the lowest energy? 5p 3d 4p 5s STUDY
3d
Which of the following subshells has the highest energy? 1s 3p 3s 2p
3p
Which orbital will have the highest energy? 5s 3s 3d 4d
4d
How many electrons are there in a Sb atom?
51
Bohr proposed that
An orbit is the fixed path of the electron around the nucleus. The energy of an electron is quantized, meaning that each orbit, also called an energy level, is associated with a discrete amount of energy. A quantum is the smallest allowed unit of energy. The energy of a quantum depends directly on the frequency of electromagnetic radiation (i.e., light). The most stable state of an atom is the one in which the electrons are in their lowest energy level, that is, the ground state. When energy is supplied, an electron absorbs energy and is transferred from its ground state to a higher energy level. The excited electron transitions back to its ground state by the emission of a photon (which can be seen as a line of light on the atom's line spectrum).
Classify the following structural characteristics of atoms into Bohr's and Rutherford's concepts of atomic structure. Drag the appropriate items to their respective bins. The mass of the electrons is very little compared to the mass of the nucleus. The electrons jump from the lowest energy level to a highest energy level when energy is supplied. The electrons tend to stay in their lowest possible energy level. The volume of the nucleus is very small compared to the total volume of the atom. The electrons can have only a certain specified amount of energy. Most of the space inside an atom is empty.
Bohr's concept The electrons jump from the lowest energy level to a highest energy level when energy is supplied. The electrons tend to stay in their lowest possible energy level. The electrons can have only a certain specified amount of energy. Rutherford's concept The mass of the electrons is very little compared to the mass of the nucleus. The volume of the nucleus is very small compared to the total volume of the atom. Most of the space inside an atom is empty.
The element with the ground state electron configuration of 1s2 2s2 2p6 3s2 3p5 is Ar Cl S Br
Cl
Rutherford proposed that
Each atom consists of a positive nucleus around which a cloud of negatively charged electrons revolve. Most of the mass is concentrated in a small, central part of the atom. The mass and all the positive charge of an atom are concentrated in a small, central region called the nucleus, and the mass of the electrons surrounding the nucleus is negligible when compared to the mass of nucleus. Most of the volume of an atom is empty space occupied by negatively charged electrons.
Classify each statement as true or false. Drag the appropriate items to their respective bins. The valence electrons of group 1A elements are in an s shell. Period 3 elements have an inner electron configuration of [Ne]. Group 8A elements have full outer principal s and p subshells. The valence electrons of group 6A elements are in the 7s subshell. Period 4 elements of six 3p electrons. The highest principal quantum number of period 3 elements is 3. Period 4 elements have an inner electron configuration of [Kr]. The highest principal quantum number of period 2 elements is 3. STUDY STUDY STUDY
True The valence electrons of group 1A elements are in an s shell. Period 3 elements have an inner electron configuration of [Ne]. Group 8A elements have full outer principal s and p subshells. Period 4 elements of six 3p electrons. The highest principal quantum number of period 3 elements is 3. False The highest principal quantum number of period 2 elements is 3. The valence electrons of group 6A elements are in the 7s subshell. Period 4 elements have an inner electron configuration of [Kr].
In which group do all atoms have one valence electron in the ground state? alkali metals alkaline earth metals halogens noble gases
alkali metals
In which group do all atoms have two valence electrons in the ground state? alkali metals alkaline earth metals halogens noble gases
alkaline earth metals
Line spectra
are generated as electrons move from one energy level to another energy level within an atom. When elements are heated (heat is a form of energy), electrons in atoms absorb the quantum of energy and are elevated to one of the higher energy levels. These excited electrons return to lower energy levels by giving up energy in the form of a photon. The energy released is seen as a discrete line on a line spectrum. Each line in the spectrum has a specific wavelength of light that corresponds to the frequency of the emitted photon (i.e., light) for that atom. Certain elements can be identified based on the light emitted by the excited atom.
The designations s, p, d, f designate different types of electrons. different electron orbitals within an energy level. valence electrons. different electron energy levels.
different electron orbitals within an energy level.
In which group do all atoms have seven valence electrons in the ground state? alkali metals alkaline earth metals halogens noble gases
halogens
In which group do all atoms have eight valence electrons in the ground state? alkali metals alkaline earth metals halogens noble gases
noble gases
The line spectra of atoms provides experimental evidence for the arrangement of electrons the organization of particles in the nucleus of atoms the number of protons all of the above
the arrangement of electrons
number of electrons, which is also equal to
the atomic number (number of protons) in a neutral atom.
Elements in the same group have the same number of neutrons. the same atomic number. the same number of electrons. the same number of valence electrons. GROUP ?
the same number of valence electrons.
formula 2n2
to find the maximum number of electrons that can exist in each energy level (shell) of an atom.
The electrons in the outermost energy level of an atom are called orbital electrons. core electrons. group electrons. valence electrons.
valence electrons.
