Without using Fig. 8.3, predict the order of increasing...

Without using Fig. $8.3$, predict the order of increasing electronegativity in each of the following groups of elements.
a. $\mathrm{Na}, \mathrm{K}, \mathrm{Rb}$
c. $\mathrm{F}, \mathrm{Cl}, \mathrm{Br}$
b. $\mathrm{B}, \mathrm{O}, \mathrm{Ga}$
d. $\mathrm{S}, \mathrm{O}, \mathrm{F}$

Key Concepts

Electronegativity

Electronegativity is a chemical property that describes an atom's ability to attract electrons in a chemical bond. Understanding electronegativity is essential for predicting bond polarity and chemical reactivity, as it determines how electrons are shared between atoms.

Periodic Trends

Periodic trends refer to the general patterns observed in properties such as electronegativity, atomic size, and ionization energy across periods and groups of the periodic table. Typically, electronegativity increases across a period from left to right and decreases down a group due to changes in effective nuclear charge and atomic radius.

Effective Nuclear Charge and Electron Shielding

Effective nuclear charge is the net positive charge experienced by electrons in an atom, accounting for both the actual nuclear charge and the shielding effect of inner electrons. A higher effective nuclear charge, which results from less shielding, leads to a stronger attraction for electrons and thus higher electronegativity.

Transcript

00:01 So in this video, we're gonna talk about question 32 from chapter eight, which says, without using figure 8.3.

00:07 Predict the order of increasing lecter negativity in each of the following groups of elements.

00:11 So first, let's talk about the general trends in the periodic table for elektra negativity.

00:17 Um, so as we go from left to right across the periodic table, what's changing? well, our nuclear charges changing, we gradually get more protons and our nucleus and increase our nuclear charge as we move from left to right across the periodic table.

00:32 And a more positively charged nucleus has a stronger pull on electrons.

00:36 So as we go from left to right, elektra negativity is increasing.

00:41 What about when we go from top to bottom? so as we move down a column in the periodic table down a group in the periodic table, um, we're gaining more shells of electrons, and our valence electrons are getting further away from the nucleus.

00:59 So the further we are from the nucleus, the more difficult it is for our nucleus to attract those electrons.

01:06 Um, and also the more shells of electrons are in between our nucleus in those outermost electrons, the more shielding effects you have.

01:15 So as we go from top to bottom, electra negativity decreases.

01:19 So we're increasing from left to right and then increasing from bottom to top as we go up the periodic table.

01:24 And as we go left to right.

01:26 So let's take that in line with me.

01:27 Answer this.

01:29 So when a.

01:30 We have sodium, potassium and rubidium.

01:33 So those air in the first call on those air alkali metals.

01:36 So we have sodium, potassium and rubidium, so we know elektra negativity increases from bottom to top of the periodic table, so rubidium must be the least.

01:45 Electra negative and sodium must be the most electra negative.

01:50 So the ordering is r b...

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