(2) a different molecular structure and the same properties
(3) the same molecular structure and different properties
(4) the same molecular structure and the same properties
Answer is: (1) a different molecular structure and different properties.
Different forms of the same element that have different properties because of different atom arrangements are called allotropes.
Carbon has many allotropes, but two most important are graphite and diamomd.
Graphite has sp2 and diamond has sp3 hybridization of carbon atoms, because of that graphite conduct electricity and diamond not.
In diamond carbon atoms are arranged in the face centered cubic crystal structure called a diamond lattice.
Diamond has very strong covalent bonds between carbon atoms and because of that it has the highest hardness and thermal conductivity of any bulk substance.
The scientist that performed the cathode ray experiment leading to the discovery of electrons is the scientist Sir Joseph John Thompson or J.J. Thompson. It was theorized after the discovery that electrons are present in the atom. In this model, the atom is composed mainly of electrons. It was describe as plum pudding because the electrons are dispersed within the atom.
John Thompson is the answer
It has three nonbonding electrons.
It has five valence electrons available for bonding.
It has five nonbonding electrons.
Answer:The answer is "It has five valence electrons available for bonding". An element's group number is equivalent to the number of valence electrons that it has. This means that since phosphorus is found on group number 5, it has 5 valence electrons that participate in bonding. It also means that it needs 3 more electrons to complete its valency.
4.5 × 10^-4.
Fusion reaction is a type of nuclear reaction where two or more nuclei combine or collide to form an element with a higher atomic number. This happens when the collision is in a very high speed. In this process, some of the matter of the fusing nuclei is converted to energy.
It's easier for elements with low ionization energy to form cations. Examples include elements in the first group of the periodic table such as Lithium and Sodium. As more electrons are removed from an atom, the ionization energy increases due to stronger electrostatic attraction.
In the context of ion formation, it is easier for an element with low ionization energy to form a positive ion or a cation. Ionization energy is the minimum amount of energy required to remove an electron from an atom in its ground state. Elements with low ionization energy can easily lose an electron to form cations as the energy required to remove the electron is not high.
For example, elements in the first group of the periodic table, such as Lithium (Li), Sodium (Na), and Potassium (K), have relatively low ionization energies and thus, easily lose their one valence electron to form cations. On the contrary, elements with high ionization energies have a stronger hold on their electrons and are thus less likely to lose an electron and form a positive ion.
Furthermore, the successive ionization energies for a single element always increase. This is because removing an electron from an already positively charged ion or cation requires more energy due to the stronger electrostatic attraction that the ion has for its electrons. This makes it progressively harder to remove additional electrons, and create ions with higher positive charges.
#SPJ3