Answer: The statement is false
Explanation:
Electrons occupy a region in atoms known as orbitals or subs hell. These orbitals include
I) S-orbital: it can occupy a maximum of two electrons
II) P-orbital: It occupies a maximum of six electrons
III) D-orbital: it occupies a maximum of ten electrons
F and G-orbitals as examples of other orbitals present.
A good illustration of the 6 electrons occupied by the P-subshell is seen in Sodium (Na) with atomic number of 11
Na = 1s2, 2S2 2p6, 3s1
Note: extra electrons are transferred to the next orbital
Answer:
BrO₃⁻ (aq) + NO₂(aq) + 4 H⁺→ Br⁻(aq) + NO₃⁻ + 2 H₂O
Explanation:
The law of conservation of matter states that since no atom can be created or destroyed in a chemical reaction, the number of atoms that are present in the reagents has to be equal to the number of atoms present in the products.
Then, you must balance the chemical equation. For that, you must first look at the subscripts next to each atom to find the number of atoms in the equation. If the same atom appears in more than one molecule, you must add its amounts.
The coefficients located in front of each molecule indicate the amount of each molecule for the reaction. This coefficient can be modified to balance the equation, just as you should never alter the subscripts.
By multiplying the coefficient mentioned by the subscript, you get the amount of each element present in the reaction.
Then, taking into account all of the above, you can determine the amount of elements on each side of the equation:
Left side: 1 Br, 5 O and 1 N
Right side: 1 Br, 3 O and 1 N
If the reaction occurs in an acidic medium:
So, balancing the oxygen:
BrO₃⁻ (aq) + NO₂(aq) → Br⁻(aq) + NO₃⁻ + 2 H₂O
Left side: 1 Br, 5 O and 1 N
Right side: 1 Br, 5 O, 1 N and 4 H
Then, balancing the hydrogens:
BrO₃⁻ (aq) + NO₂(aq) + 4 H⁺→ Br⁻(aq) + NO₃⁻ + 2 H₂O
Left side: 1 Br, 5 O, 1 N and 4 H
Right side: 1 Br, 5 O, 1 N and 4 H
You can see that you have the same amount on each side of the reaction. So the reaction is balanced.
B. remains constant within a period
C. decreases as you move from left to right across a period
D. increases as you move from left to right across a period
Option C, decreases as you move from left to right across a period
As you move from left to right across a period, the atoms get more and more protons. These protons pull on the electrons, making the atoms progressively smaller and smaller because of the increasing pull.
Atomic size generally increases as you move from top to bottom within a group due to increase in the principal quantum number. However, atomic size generally decreases as you move from left to right across a period, as the added protons and electrons increase the effective nuclear charge and pull the electrons in closer.
In the context of atomic size on the periodic table, there are two primary trends to notice: Atomic size generally decreases as you move from left to right across a period. This happens because as we move from left to right, we add a proton to the nucleus and an electron to the valence shell with each successive element, thereby increasing the effective nuclear charge and pulling the electrons in tighter to the nucleus.
Atomic size generally increases as you move from top to bottom within a group. This is due to the increase in the principal quantum number, causing the atomic radius to grow as there are more electron shells.
These observations come from understanding the electronic structure of elements and how they influence the properties like atomic size, ionization energies and electron affinities that vary periodically as the electronic structure of the elements changes.
#SPJ12
(2) equal to the number of protons gained
(3) less than the number of electrons gained
(4) less than the number or protons gained