0
What are three examples of elements with unpredictable electron configurations?
Wiki User
∙ 13y ago
Copper and Chromium have 1 electron in the 4s subshell, and 5 and 10 in the 3d subshell respectively. You needn't know beyond that until University.
Wiki User
∙ 13y ago
- Chromium: Chromium typically forms a half-filled d5 configuration (4s1 3d5) instead of a fully-filled d4 configuration (4s2 3d4) due to the increased stability associated with the half-filled d orbital.
- Copper: Copper prefers to have a full d10 configuration (4s1 3d10) instead of a partially filled d9 configuration (4s2 3d9) as it increases stability.
- Silver: Silver can have an electron configuration of [Kr] 4d10 5s1 instead of the expected [Kr] 4d9 5s2 due to the stability associated with the fully-filled 4d orbital.
Add your answer:
Earn +20 pts
What is the name of an element with a full electron shell?
An element with a full electron shell is called a noble gas. These elements have stable electron configurations and do not easily form chemical bonds with other elements. Examples include helium, neon, and argon.
Which elements would likely for anions with a -1 charge?
Elements in group 17 of the periodic table, known as the halogens, are likely to form anions with a -1 charge. Examples include fluorine, chlorine, and iodine. These elements have 7 valence electrons and tend to gain one electron to achieve a stable electron configuration.
What do the blue colored elements on the periodic table indicate?
The blue colored elements on the periodic table indicate the noble gases. These elements are typically unreactive and have a full outer electron shell, making them stable. Examples include helium, neon, and argon.
What are macroscopic elements?
Macroscopic elements are elements that can be seen with the naked eye or analyzed using macroscopic techniques, such as visual inspection or simple laboratory tests. Examples include iron, copper, and aluminum. These elements are distinct from microscopic elements, which require more sophisticated techniques, such as electron microscopy, to analyze.
What are elements that don't react rapidly with other elements called?
Inert gases, also known as noble gases, are elements that do not react rapidly with other elements because they have a full outer electron shell, making them stable. Examples include helium, neon, and argon.
What are the examples of elements with predictable electron configurations?
Noble gases have predictable electron configurations as they have completely filled outer electron shells (e.g. helium, neon). Transition metals also have predictable electron configurations based on their position on the periodic table and electron filling rules (e.g. iron, copper).
What elements has a ground-state electron configuration different from the predicted one?
Transition metals have ground-state electron configurations that differ from the predicted ones due to the exchange of electrons between the ns and (n-1)d subshells. This exchange stabilizes the d orbitals, leading to configurations that are closer to half-filled or fully filled d subshells. Examples include chromium ([Ar] 3d^5 4s^1) and copper ([Ar] 3d^10 4s^1).
What are examples of elements with one as their valency i.e.give examples of monovalent elements.?
Examples of monovalent elements include hydrogen, sodium, and potassium. These elements have one valence electron, which allows them to easily form ions with a +1 charge.
Argon Helium and Neon are examples of?
Noble gases. They are colorless, odorless, and have low chemical reactivity due to their stable electron configurations. They are commonly used in applications such as lighting, cooling, and insulation.
What is the name of an element with a full electron shell?
An element with a full electron shell is called a noble gas. These elements have stable electron configurations and do not easily form chemical bonds with other elements. Examples include helium, neon, and argon.
Which elements are likely to combine chemically?
Elements with similar electronegativities and valence electron configurations are likely to combine chemically. This is because they tend to form stable compounds by either sharing electrons (covalent bonding) or transferring electrons (ionic bonding) to achieve a more stable electron configuration. Examples include hydrogen and oxygen combining to form water (H2O) through covalent bonding, or sodium and chlorine combining to form sodium chloride (NaCl) through ionic bonding.
Which elements would likely for anions with a -1 charge?
Elements in group 17 of the periodic table, known as the halogens, are likely to form anions with a -1 charge. Examples include fluorine, chlorine, and iodine. These elements have 7 valence electrons and tend to gain one electron to achieve a stable electron configuration.
Which atoms form ionic compound?
Atoms that form ionic compounds typically involve elements with large differences in electronegativity. This results in one atom donating electrons to another to achieve stable electron configurations. Common examples include metals like sodium donating electrons to nonmetals like chlorine to form sodium chloride.
Were the Greek gods good examples of leaders?
They were not, as they were often moody and unpredictable.
What are the example of inner transition element?
Examples of inner transition elements include lanthanides (elements 57-71) and actinides (elements 89-103) located at the bottom of the periodic table. These elements have partially filled f-orbitals and exhibit unique chemical properties due to their electron configurations. Some common inner transition elements include cerium, uranium, and plutonium.
What compounds form single covalent bonds?
Elements in group 17 need one electron to gain a stable electron configuration. Two atoms of the same element or two elements in this family forms compounds with a single covalent bond. Examples are chlorine, bromine or iodine chloride.
Which elements have positive electron gain enthalpy?
Fluorine, oxygen, nitrogen, and chlorine are examples of elements that typically have positive electron gain enthalpy. This means that they tend to release more energy when they lose an electron than when they gain an electron due to their high electron affinities.
