It is so hard i do not get it
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your friend has to plan an experiment for a science fair. He asked for your help. His topic is "The Strongest Cloth for Backpacks." What variables must the experinemt include? What variables must be controlled?
B. Density
C. Melting point
D. Color
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Answer : The properties which would be the same among isotopes of the same element are Flammability and Color
Explanation :
Isotopes are the elements that have same number of electrons and protons but they differ in number of neutrons.
The chemical properties of an element are determined by its valence electrons and since isotope have same number of electrons, they have similar chemical properties.
But isotopes have different number of neutrons. Neutrons are the subatomic particles which are present in the nucleus. They are charge less particles and they have mass. Therefore when the elements have different number of neutrons, their atomic masses differ.
As a result, isotopes have different mass related physical properties.
Let us discuss the given properties now
1) Flammability : Flammability in simple words means the ability of the substance to catch fire or the ability to burn. This is mainly dependent on the reactivity which is in turn dependent on the number of electrons.
Since the isotopes have same number of electrons, they show similar flammability.
2) Density : Density is defined as mass per unit volume. This property involves mass and we know that isotopes have different masses. Therefore they have different densities too.
3) Melting point : Melting point is a physical property which is mainly dependent on the molecular weight of the substance. Since isotopes have different masses, they tend to show different melting points.
4) Color : The color of the element is mainly dependent on the arrangement of electrons around the nucleus. Isotopes have same number of electrons which means the arrangement would also be the same. Therefore the isotopes of the same element do not show different colors.
The properties which would be same among isotopes of the same element are
1) Flammability
4) Color
Answer: D. Color
Explanation: Founders Educere answer.
So much for expert verified^^ smh
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B electrons move to higher energy levels
** C electrons are gained by an atom in
D. člectrons fall bàok to lower energy levels
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Answer:
option d= electrons fall back to the lower energy levels
Explanation:
Excitation:
When the energy is provided to the atom the electrons by absorbing the energy jump to the higher energy levels. This process is called excitation. The amount of energy absorbed by the electron is exactly equal to the energy difference of orbits.
De-excitation:
When the excited electron fall back to the lower energy levels the energy is released in the form of radiations. this energy is exactly equal to the energy difference between the orbits. The characteristics bright colors are due to the these emitted radiations. These emitted radiations can be seen if they are fall in the visible region of spectrum.
Fluorescence:
In fluorescence the energy is absorbed by the electron having shorter wavelength and high energy usually of U.V region. The process of absorbing the light occur in a very short period of time i.e. 10 ∧-15 sec. During the fluorescence the spin of electron not changed.
The electron is then de-excited by emitting the light in visible and IR region. This process of de-excitation occur in a time period of 10∧-9 sec.
Phosphorescence:
In phosphorescence the electron also goes to the excitation to the higher level by absorbing the U.V radiations. In case of Phosphorescence the transition back to the lower energy level occur very slowly and the spin pf electron also change.
Final answer:
The characteristic color (spectrum) of an element is produced when its electrons fall back to lower energy levels. They absorb energy to jump to a higher level, then emit it in the form of light of a specific wavelength when returning to their original or lower level.
Explanation:
The characteristic bright-line spectrum (color) of an element is produced when electrons fall back to lower energy levels (Option D). This process is part of the quantum mechanical model of the atom, particularly in the field of spectroscopy. Each element possesses unique energy levels. When an electron in an atom absorbs energy, it jumps to a higher energy level. When the electron returns to its original or lower energy level, it emits energy in the form of light of a specific wavelength. This is viewed as a unique color in the spectrum.
Learn more about Electron Energy Levels here:
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