A compound accepts electrons from another substance to form a covalent bond. The compound acts as a Lewis base.
<h3>What are the most common acid-base theories?</h3>
- Arrhenius: acids release H⁺ and bases release OH⁻.
- Bronsted-Lowry: acids donate H⁺ and bases accept H⁺.
- Lewis: acids accept electrons and bases donate electrons.
A compound accepts electrons from another substance to form a covalent bond. Which term best describes this compound’s behavior?
- Lewis acid. YES.
- Arrhenius base. NO, because OH⁻ is not involved.
- Bronsted-Lowry acid. NO, because H⁺ is not involved.
- Bronsted-Lowry base. NO, because H⁺ is not involved.
A compound accepts electrons from another substance to form a covalent bond. The compound acts as a Lewis base.
Learn more about Lewis acid-base theory here: brainly.com/question/7031920
Answer:
29.85°C
Explanation:
0°K is absolute zero. That is is same as -273.15°C.
To find C, subtract 273.15 from the temperature in °K.
303K - 273.15°C = <em><u>29.85°C</u></em>
It would be C because you would do m divided by s squared and you would get 0.11 but you would round it to 0.12
Answer: SnO2 + 2 H2 = Sn + 2 H2O
Explanation: I used a balance equation website. It's called WebQC if you want to check it out for future help.
