Which do not obey the octet rule?
Check all that apply.
NO
BF3
ICl2^-
OPBr3
XeF4
An explanation would be appreciated, thanks.
Never mind, I got it.
All of them. They all have an odd number of valence electrons.
Well, well, well, let's dig into this question with a touch of humor!
The octet rule is like a strict bouncer at a club, only allowing up to 8 electrons to fill the outermost shell of an atom. So, who are the party animals that don't want to follow the rule? Here they are:
1. NO: Nitric Oxide. This mischievous molecule has an odd number of valence electrons, so it crashes the octet party.
2. ICl2^-: This is where things get interesting! ICl2^- is a polyatomic ion consisting of iodine and chlorine. Iodine, being unfazed by rules, happily accepts 2 more electrons, making it an exception to the octet rule.
3. XeF4: Oh, XeF4, you cheeky little compound! Xenon, the noble gas, despite having the potential party capacity for 8 electrons, dives into the octet rule with a whopping 12 electrons. It just loves to break the rules!
Now, on to the other contenders:
1. BF3: Boron trifluoride knows how to behave, following the octet rule perfectly with 6 electrons around it.
2. OPBr3: This one plays nice too! OPBr3, also known as phosphorous tribromide oxide, obeys the octet rule as well.
So, there you have it! The rule breakers are NO, ICl2^-, and XeF4. They just can't resist their rebellious nature!
The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with eight valence electrons. Let's examine each molecule or ion and determine if they obey the octet rule:
1. NO: This molecule consists of one nitrogen atom (N) bonded to one oxygen atom (O). Nitrogen has 5 valence electrons and oxygen has 6, so the total number of valence electrons in NO is 11. Since it is a stable molecule with only one double bond, it does not obey the octet rule.
2. BF3: This molecule consists of one boron atom (B) bonded to three fluorine atoms (F). Boron has 3 valence electrons, and fluorine has 7. The total valence electron count of BF3 is 24, which satisfies the octet rule.
3. ICl2^-: This ion consists of one iodine atom (I) bonded to two chlorine atoms (Cl) and an extra electron. Iodine has 7 valence electrons, chlorine has 7, and the additional electron gives it a total of 24 valence electrons. This ion obeys the octet rule because it has 8 valence electrons around the central iodine atom.
4. OPBr3: This molecule consists of one oxygen atom (O) bonded to one phosphorus atom (P) and three bromine atoms (Br). Oxygen has 6 valence electrons, phosphorus has 5, and bromine has 7. The total valence electron count of OPBr3 is 34, which exceeds the octet rule.
5. XeF4: This molecule consists of one xenon atom (Xe) bonded to four fluorine atoms (F). Xenon has 8 valence electrons, and fluorine has 7. The total valence electron count of XeF4 is 36, which exceeds the octet rule.
So, the molecules that do not obey the octet rule are NO, OPBr3, and XeF4.
To determine which of the given molecules do not obey the octet rule, let's first understand what the octet rule is.
The octet rule states that atoms tend to gain, lose, or share electrons in order to have a full set of eight valence electrons in their outermost energy level. This applies to most elements, especially those in the main group elements of the periodic table.
Let's analyze each molecule to see if they follow the octet rule:
1. NO:
Nitrogen (N) has 5 valence electrons, and Oxygen (O) has 6 valence electrons. When they form a bond, Nitrogen can share three electrons with Oxygen, resulting in a total of 8 electrons around the nitrogen atom. Therefore, NO obeys the octet rule.
2. BF3:
Boron (B) has 3 valence electrons, and Fluorine (F) has 7 valence electrons. When they form bonds, each fluorine atom can share one electron with boron. This results in a total of 6 electrons around the boron atom, fewer than the octet rule requires. Therefore, BF3 does not obey the octet rule.
3. ICl2^-:
Iodine (I) has 7 valence electrons, Chlorine (Cl) has 7 valence electrons, and the negative charge adds one more electron for a total of 8. When they form bonds, each chlorine atom can share one electron with iodine. This results in a total of 8 electrons around the iodine atom, which obeys the octet rule. Therefore, ICl2^- obeys the octet rule.
4. OPBr3:
Oxygen (O) has 6 valence electrons, Phosphorous (P) has 5 valence electrons, and Bromine (Br) has 7 valence electrons. When they form bonds, each oxygen atom can share two electrons with phosphorous, and each bromine atom can share one electron with phosphorous. This results in a total of 10 electrons around the phosphorous atom, more than the octet rule requires. Therefore, OPBr3 does not obey the octet rule.
5. XeF4:
Xenon (Xe) has 8 valence electrons, and Fluorine (F) has 7 valence electrons. When they form bonds, each fluorine atom can share one electron with xenon. This results in a total of 8 electrons around the xenon atom, which obeys the octet rule. Therefore, XeF4 obeys the octet rule.
Based on this analysis, the molecules that do not obey the octet rule are:
- BF3
- OPBr3