On one graph, plot the effective nuclear charge (shown in parentheses) and atomic radius (see Figure 7.6 ) versus atomic number for the second-period elements: Li ( 1 .28 ) , Be ( 1 .91 ) , B ( 2 .42 ) , C ( 3 .14 ) , N ( 3 .83 ) , O ( 4 .45 ) , F ( 5 .10 ) , Ne ( 5 .76 ) . Comment on the trends.
On one graph, plot the effective nuclear charge (shown in parentheses) and atomic radius (see Figure 7.6 ) versus atomic number for the second-period elements: Li ( 1 .28 ) , Be ( 1 .91 ) , B ( 2 .42 ) , C ( 3 .14 ) , N ( 3 .83 ) , O ( 4 .45 ) , F ( 5 .10 ) , Ne ( 5 .76 ) . Comment on the trends.
Solution Summary: The author explains that effective nuclear charge increases across a period due to increase in number of valence electrons.
On one graph, plot the effective nuclear charge (shown in parentheses) and atomic radius (see Figure 7.6) versus atomic
number for the second-period elements:
Li
(
1
.28
)
, Be
(
1
.91
)
, B
(
2
.42
)
, C
(
3
.14
)
, N
(
3
.83
)
, O
(
4
.45
)
, F
(
5
.10
)
, Ne
(
5
.76
)
. Comment on the trends.
Definition Definition Number of protons in the nucleus of an atom. It uniquely identifies an element, as the number of protons determines the element's properties. The periodic table of elements is arranged based on increasing atomic numbers, allowing scientists to easily locate and study elements.
(a) Describe the trends of atomic size and ionization energy, respectively, in the Periodic Table:
(1) from left to right across a period, and (ii) from top to bottom down a group.
(b) Rank the following elements: Na, Mg, Al, and K, in increasing order of: (i) atomic size; (ii) ionization
energy, and (iii) reactivity.
(c) Rank the following elements: F, CI, Br and I, in increasing order of: (i) atomic size; (ii) electron
affinity, (iii) electronegativity, and (iv) reactivity.
(a) Rank elements: Na, Mg, Al, and K, in increasing order of: (i) atomic size; (ii) ionization energy, and (iii) reactivity. (b) Explain why atomic size decreases from left to right, but increases from top to bottom; (c) Explain why ionization energy increases from left to right, but decreases from top to bottom; (d) Explain why the reactivity of alkali metals (Group-1) increases from top to bottom, where as the reactivity of halogen (Group-17) decreases from top to bottom.
I hate that I always have to waste my limited quanitty of questions for follow ups for a decent explaination.I don't understand.It must be in a +3 state?Why?F has a -1 charge, that means it would have:9p 10e due to it's 18.99 mass.and since the charge is -1, that would imply 10e.That means I need an element with +1 charge to balance, but also should have 12e.Mn has a charge of +2 generally, but it can have +3.I was given zero understanding of how it could be any element with a +1 charge that has those numbers of electrons.I need help understanding this.
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