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How much energy does the electron have initially in the n equals 4 excited state?
The energy of an electron in the n equals 4 excited state can be calculated using the formula E = -13.6eV/n^2. Plugging n = 4 into the formula, the energy of the electron in the n equals 4 excited state would be -2.125 eV.
If a Hypothetical atom has energy levels from lowest to highest as n equals 1 n equals 2 and n equals 3 For an electron in this atom to move from n equals 1 to n equals 3 orbit the electron must?
Absorb appx 12.1eV (electron Volts) of energy. Energy of 1st level is -13.6eVEnergy of 3rd level is -1.5eV Hence, energy required = 13.6 - 1.5 = 12.1 eV
How much energy is required to cause an electron in hydrogen to move from the n 3 state to the n 2 state?
The energy required to move an electron from the n=3 to n=2 state in hydrogen is approximately 10.2 eV (electron volts). This energy corresponds to the difference in energy levels between the two states and is typically provided in the form of a photon during absorption or emission processes.
What is the magnitude of the electric force on an electron placed in a uniform electric field of 610 N per C?
The magnitude of the electric force on an electron placed in a uniform electric field is given by the equation F = qE, where F is the force, q is the charge of the electron, and E is the electric field strength. The charge of an electron is approximately 1.6 x 10^-19 C. Therefore, the magnitude of the electric force on an electron in a 610 N/C electric field is (1.6 x 10^-19 C)(610 N/C) = 9.76 x 10^-17 N.
Which quantum number represents the main energy level of an electron?
The principal quantum number (n) represents the main energy level of an electron in an atom. It determines the energy level and distance of the electron from the nucleus.
How do the valence electron configurations of the alkali metals compare with others?
The valance electron configuration is the same in each at ns1 where n = the period number.
Which pair of atoms will have the same valence-shell electron configuration Se and Te Sr and Cs N and O H and He?
Se and Te will have the same valence-shell electron configuration as they are both in the same group (group 16) and have 6 valence electrons. Sr and Cs will have different valence-shell electron configurations as Sr is in group 2 with 2 valence electrons and Cs is in group 1 with 1 valence electron. N and O will have different valence-shell electron configurations as N has 5 valence electrons while O has 6. H and He will have different valence-shell electron configurations as H has 1 valence electron and He has 2.
How do the valence electrons configurations of the alkali metals compare with each other?
The valance electron configuration is the same in each at ns1 where n = the period number.
Why do alkali metals tend to lose 1 valence electron?
Every alkali metal has only one electron in the outermost energy level. They give it away to form monopositive ions which have stable electron configurations ending with ns2 np6 (where n is a counting number between 2 and 7 inclusive).
WhAt is the ending of the electron configuration of each element in group 4?
Elements in Group 4 end their electron configurations with 4s2 4p2. This is because they have 4 valence electrons, with the last two electrons occupying the s-subshell (4s) and the p-subshell (4p) completing the outermost energy level.
What is the electrons arrangement in sodium azide?
In sodium azide (NaN₃), the electron arrangement can be understood by considering the electron configurations of the individual atoms involved. Sodium (Na) has an electron configuration of [Ne] 3s¹, while nitrogen (N) has an electron configuration of [He] 2s² 2p³. When sodium donates its electron to form the Na⁺ cation, and nitrogen accepts these electrons to form the N₃⁻ anion, the overall electron arrangement in sodium azide involves the transfer of electrons to achieve a stable octet configuration for each atom.
When compared with an electron for which n equals 2 an electron for which n equals 4 has more?
Energy
When a hydrogen electron transitions from n equals 1 to n equals 4 is the energy of electron increased or decreased?
decreased
Between H2NNH2 and HNNH which molecule has the stronger N-N bond?
The N-N bond in H2NNH2 (hydrazine) is stronger than in HNNH (diazene). This is because hydrazine has a longer N-N bond length, allowing for more electron-electron repulsion, which strengthens the bond. Diazene has a shorter N-N bond with less electron-electron repulsion, resulting in a weaker bond.
What is the valence electron configuration of each element in group 1?
All elements in group 1 have 1 valence electron.
Why is a shorter wavelength of light emitted when an electron falls from n equals 4 to n equals 1 than when an electron falls from n equals 2 to n equals 1?
Shorter wavelength = more energy. The farther the electron falls, the more energy that will be emitted.
What element electron configurations would represent a halogen?
The halogens are is group VII (17), and thus they all have 7 valence electrons. These will be located in different energy levels for the different halogens, but since they are all also p-block elements, they will all have ns^2 np^5 electron configurations, where n is the period number. Examples: Cl will be [Ne] 3s^2 3p^5 and Br will be [Ar] [Ar] 4s2 3d10 4p5 (note the inclusion of the d-block electrons for Br).
