Arsenic is atomic number 33 and has 5 valence electrons.
Method for finding valence electrons: All electrons are arranged in orbital shells. The inner shell can hold up to 2 electrons. The second shell holds up to 8. The third shell holds up to 18 and so on. The outer shell holds the valence electrons. To find out how many there are, count the electrons in the inner shells 2+8+18 = 28, in this case, and subtract them from the 33 electrons that Arsenic has: 33 - 28 = 5 valence electrons.
The element with four valence electrons, showing properties of both metals and nonmetals, and having 14 protons is silicon. Silicon can behave as a semiconductor, exhibiting properties of both metals and nonmetals depending on the specific conditions.
silicon
Arsenic.
Elements share similar characteristics because they have the same number of electrons in their outermost energy level, which determines their chemical properties. This similarity is due to their placement in the periodic table, where elements in the same group have the same number of valence electrons. These shared characteristics allow elements to react in similar ways and form similar types of compounds.
Valence electrons are the electrons that account for many of the chemical and physical properties of elements. These are the electrons in the outermost energy level of an atom and are involved in chemical bonding and reactions. The number of valence electrons determines an element's reactivity and ability to form compounds.
The answer is "the electron." "Valance Electron" is a more specific and correct answer.
Nonmetals can complete the octet rule by gaining electrons to achieve a stable electron configuration with 8 valence electrons. This can be achieved through forming covalent bonds with other nonmetals, sharing electrons to reach octet stability. Additionally, nonmetals can also gain electrons to reach a stable noble gas configuration, such as gaining 2 electrons to achieve an outer shell configuration like a noble gas.
Because they have similar chemical properties. The reason they have similar chemical properties is because they have the same number of valence electrons. The differences are caused by them having different masses and because the larger elements have their valence electrons "screened" more from the nucleus by electrons in lower energy levels.
These are the chemical properties.
Valence electrons are the electrons that account for many of the chemical and physical properties of elements. These are the electrons in the outermost energy level of an atom and are involved in chemical bonding and reactions. The number of valence electrons determines an element's reactivity and ability to form compounds.
The answer is "the electron." "Valance Electron" is a more specific and correct answer.
Elements in a group have the same number of valence electrons because they have similar electron configurations, as they are in the same column of the periodic table. Valence electrons are the outermost electrons of an atom, and they determine the element's chemical properties. Elements in the same group have the same number of valence electrons, leading to similar reactivity and bonding behavior.
The number of protons in the atomic nucleus determines the properties of an element. Every element has its own unique number of protons, called its atomic number, which is displayed on the periodic table. The elements are arranged in order of increasing atomic number on the periodic table.
Elements share similar characteristics because they have the same number of electrons in their outermost energy level, which determines their chemical properties. This similarity is due to their placement in the periodic table, where elements in the same group have the same number of valence electrons. These shared characteristics allow elements to react in similar ways and form similar types of compounds.
If you are talking about elements, they are electrons.
Because they have similar chemical properties. The reason they have similar chemical properties is because they have the same number of valence electrons. The differences are caused by them having different masses and because the larger elements have their valence electrons "screened" more from the nucleus by electrons in lower energy levels.
No, radioactivity refers to the emission of particles or energy from the nucleus of an atom, while acidity refers to the concentration of hydrogen ions in a solution. These are two separate properties and being radioactive does not make a substance acidic.
With each additional period, there is an additional energy level, which means that the outermost electrons are farther away from the nucleus of the atom. This means that the attractive force of the positively charged nucleus is less, so it takes less energy to remove an electron from an atom in the third energy level than it does from an atom in the second energy level. Therefore, the elements in the third period have lower ionization energies than elements in the second period.
The properties of the atom
The properties of the atom