For each of the following atomic numbers, use the periodic table to write the formula (including

For each of the following atomic numbers, use the periodic...

Key Concepts

Periodic Table and Group Trends

The periodic table is organized into groups and periods that reflect recurring chemical properties. Elements in the same group often form ions with similar charges due to having the same number of valence electrons. This trend allows us to predict the likely charge an element will adopt in ionic compounds based on its position in the periodic table.

Formation of Simple Ions

When atoms form simple ions, they do so by gaining or losing electrons to achieve a stable electron arrangement, typically resembling that of a noble gas. Metals generally lose electrons to form positively charged cations, while nonmetals tend to gain electrons to become negatively charged anions. This process is crucial for the formation of ionic compounds.

Charge of Ions and Oxidation States

An ion's charge is determined by the balance between the number of protons and electrons. In the context of ionic compounds, these charges are often referred to as oxidation states. Recognizing common oxidation states for elements—especially those found in specific groups on the periodic table—enables us to accurately predict the formulas of simple ions.

Using Atomic Numbers to Identify Elements

The atomic number of an element indicates the number of protons in its nucleus and helps in identifying the element on the periodic table. Once an element is identified, its group and position provide essential information about its electron configuration and the typical ionic charge it will carry when forming ionic compounds.

Transcript

00:01 So this video we're gonna talk about question 74 from chapter two, which says, for each of the following atomic numbers used the periodic table to write the formula, including the charge for the simple eye on the element is most likely to form and ionic compounds.

00:17 So in a way, we're given on atomic number of 13.

00:22 So let's look in the periodic table for the moment.

00:25 With an atomic number are 13.

00:28 So the element atomic number 13 is aluminum over here.

00:33 Um, and, uh, it's kind of an exception.

00:37 Most rules, but aluminum usually takes a positive three charge when it becomes an eye on.

00:44 And i think unease e way to remember that is that aluminum, zinc and silver the charges that they usually take when they become ions are plus three plus two in plus one.

00:56 So we have 3 to 1 on this little staircase from aluminum, zinc to silver.

01:01 So +321 is a good way of remembering that, um, so for this one, we have et al three plus, um, and then and b, we want the element with an atomic number of 34.

01:23 So the element with an atomic number of 34 is selenium is over here.

01:30 Um, and how do we know what charge cellini, um, prefers to take when it becomes an eye on, um, well, the most useful thing to think about when you're trying to determine this.

01:41 There are exceptions to this, but in general, are all of the elements want to have the noble gas configuration? it's just the most stable on electronic configuration.

01:54 So they wanna have the school electron shell that corresponds to the electron configuration of these elements.

01:59 It's on the far right column of the periodic table.

02:03 Um, so in order to do that, they either gain or lose electrons.

02:08 So, for example, selenium would gain two electrons in order to have the electronic configuration matching krypton, which would be more stable.

02:19 Um, so cellini was gonna take a minus two charge, but you can see elements that are on the left hand side of the periodic table.

02:27 It would be easier to lose electrons rather than gain them in order to reach the noble gas configuration that's closest to them.

02:35 That's, um, requires adding or removing the fewest number of electrons.

02:41 But anyway, and for b, we have cellini.

02:44 Um, so we have s e.

02:45 And we have a minus two charge.

02:47 So us e to minus, um, and see, we have an atomic number of 56...

Please give Ace some feedback