genchem hashtag performance

#genchem encapsulates chemistry concepts, experiments, educational content, engaging visuals, student collaboration, fun learning, science curiosity, interactive quizzes, lab demonstrations, study tips, problem-solving, textbook summaries, and community discussions for aspiring chemists.

I love it so much- it might seem silly but honestly seeing stuff like this on TV might inspire a kid or two to check out chemistry, or at least have a little bit more fun in lab #chemistry #fyp #chemist #onceuponatime #ouat #chem #chemlab #rainbow #reginamills #drjeckyll #orgo #ochem #genchem

I love it so much- it might seem silly but honestly seeing stuff like this on TV might inspire a kid or two to check out chemistry, or at least have a little bit more fun in lab #chemistry #fyp #chemist #onceuponatime #ouat #chem #chemlab #rainbow #reginamills #drjeckyll #orgo #ochem #genchem

coordinated like ligands locked in alien by Dexterous Animation "The Pauli Exclusion Principle states that, in an atom or molecule, no two electrons can have the same four electronic quantum numbers. As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins. This means if one electron is assigned as a spin up (+1/2) electron, the other electron must be spin-down (-1/2) electron. Electrons in the same orbital have the same first three quantum numbers, e.g., n=1 , l=0, ml=0 for the 1s subshell. Only two electrons can have these numbers, so that their spin moments must be either ms=−1/2 or ms=+1/2. If the 1s orbital contains only one electron, we have one ms value and the electron configuration is written as 1s1 (corresponding to hydrogen). If it is fully occupied, we have two ms values, and the electron configuration is 1s2 (corresponding to helium). As you can see, the 1s and 2s subshells for beryllium atoms can hold only two electrons and when filled, the electrons must have opposite spins. Otherwise they will have the same four quantum numbers." #chemistry #genchem #chemistrymajor #premed #pchem #ochem

coordinated like ligands locked in alien by Dexterous Animation "The Pauli Exclusion Principle states that, in an atom or molecule, no two electrons can have the same four electronic quantum numbers. As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins. This means if one electron is assigned as a spin up (+1/2) electron, the other electron must be spin-down (-1/2) electron. Electrons in the same orbital have the same first three quantum numbers, e.g., n=1 , l=0, ml=0 for the 1s subshell. Only two electrons can have these numbers, so that their spin moments must be either ms=−1/2 or ms=+1/2. If the 1s orbital contains only one electron, we have one ms value and the electron configuration is written as 1s1 (corresponding to hydrogen). If it is fully occupied, we have two ms values, and the electron configuration is 1s2 (corresponding to helium). As you can see, the 1s and 2s subshells for beryllium atoms can hold only two electrons and when filled, the electrons must have opposite spins. Otherwise they will have the same four quantum numbers." #chemistry #genchem #chemistrymajor #premed #pchem #ochem

A brief explanation of how the acidity vs bond strength of an X-H bond are not correlated/the same. Stems from one referring to heterolytic cleavage to get X- and H+, while the other refers to homolytic cleavage. If people are interested in the MO theory explanation lmk:)! #stem #chem #chemistrytest #science #genchem #bonds #ochem #pka #chemistry

A brief explanation of how the acidity vs bond strength of an X-H bond are not correlated/the same. Stems from one referring to heterolytic cleavage to get X- and H+, while the other refers to homolytic cleavage. If people are interested in the MO theory explanation lmk:)! #stem #chem #chemistrytest #science #genchem #bonds #ochem #pka #chemistry

don't treat them like a bonding orbital if they act like an antibonding orbital source sigma and pi bonds by Chemistry Student on yt "Electrons that spend most of their time between the nuclei of two atoms are placed into the bonding orbitals, and electrons that spend most of their time outside the nuclei of two atoms are placed into antibonding orbitals. This is because there is an increasing in electron density between the nuclei in bonding orbitals, and a decreasing in electron density in antibonding orbitals (Chang 459). Placing an electron in the bonding orbital stabilizes the molecule because it is in between the two nuclei. Conversely, placing electrons into the antibonding orbitals will decrease the stability of the molecule. Electrons will fill according to the energy levels of the orbitals. They will first fill the lower energy orbitals, and then they will fill the higher energy orbitals. If a bond order of zero is obtained, that means that the molecule is too unstable and so it will not exist." #chemistry #genchem #electrons #orbitals #sigma #chem

don't treat them like a bonding orbital if they act like an antibonding orbital source sigma and pi bonds by Chemistry Student on yt "Electrons that spend most of their time between the nuclei of two atoms are placed into the bonding orbitals, and electrons that spend most of their time outside the nuclei of two atoms are placed into antibonding orbitals. This is because there is an increasing in electron density between the nuclei in bonding orbitals, and a decreasing in electron density in antibonding orbitals (Chang 459). Placing an electron in the bonding orbital stabilizes the molecule because it is in between the two nuclei. Conversely, placing electrons into the antibonding orbitals will decrease the stability of the molecule. Electrons will fill according to the energy levels of the orbitals. They will first fill the lower energy orbitals, and then they will fill the higher energy orbitals. If a bond order of zero is obtained, that means that the molecule is too unstable and so it will not exist." #chemistry #genchem #electrons #orbitals #sigma #chem

follow for more chem study guides "The postulates of the kinetic molecular theory of gases ignore both the volume occupied by the molecules of a gas and all interactions between molecules, whether attractive or repulsive. In reality, however, all gases have nonzero molecular volumes. Furthermore, the molecules of real gases interact with one another in ways that depend on the structure of the molecules and therefore differ for each gaseous substance. In this section, we consider the properties of real gases and how and why they differ from the predictions of the ideal gas law. We also examine liquefaction, a key property of real gases that is not predicted by the kinetic molecular theory of gases. For an ideal gas, a plot of PV/nRT versus P gives a horizontal line with an intercept of 1 on the PV/nRT axis. Real gases, however, show significant deviations from the behavior expected for an ideal gas, particularly at high pressures (part (a) in Figure 11.1.1 ). Only at relatively low pressures (less than 1 atm) do real gases approximate ideal gas behavior (part (b) in Figure 11.1.1 ). Real gases also approach ideal gas behavior more closely at higher temperatures, as shown in Figure 11.1.2 for N2. Why do real gases behave so differently from ideal gases at high pressures and low temperatures? Under these conditions, the two basic assumptions behind the ideal gas law—namely, that gas molecules have negligible volume and that intermolecular interactions are negligible—are no longer valid." #genchem #pchem #chemistry #physics #gaslaws #pvnrt #science #chemistrymajor

follow for more chem study guides "The postulates of the kinetic molecular theory of gases ignore both the volume occupied by the molecules of a gas and all interactions between molecules, whether attractive or repulsive. In reality, however, all gases have nonzero molecular volumes. Furthermore, the molecules of real gases interact with one another in ways that depend on the structure of the molecules and therefore differ for each gaseous substance. In this section, we consider the properties of real gases and how and why they differ from the predictions of the ideal gas law. We also examine liquefaction, a key property of real gases that is not predicted by the kinetic molecular theory of gases. For an ideal gas, a plot of PV/nRT versus P gives a horizontal line with an intercept of 1 on the PV/nRT axis. Real gases, however, show significant deviations from the behavior expected for an ideal gas, particularly at high pressures (part (a) in Figure 11.1.1 ). Only at relatively low pressures (less than 1 atm) do real gases approximate ideal gas behavior (part (b) in Figure 11.1.1 ). Real gases also approach ideal gas behavior more closely at higher temperatures, as shown in Figure 11.1.2 for N2. Why do real gases behave so differently from ideal gases at high pressures and low temperatures? Under these conditions, the two basic assumptions behind the ideal gas law—namely, that gas molecules have negligible volume and that intermolecular interactions are negligible—are no longer valid." #genchem #pchem #chemistry #physics #gaslaws #pvnrt #science #chemistrymajor

I made these for the ochem class i’m a learning assistant for so I figured i’d share them for anyone who’s just starting ochem or needs reminders! #ochem #chemistry #chem #chemnotes #notes #student #chemical #chemist #organicchemistry #orgo #organicchemistrytutor #uni #studywithme #studymotivation #studentlife #student #biochemist #biochemistry #biochem #biochemistrymajor #chemistrymajor #chemteacher #chemistrylab #organic #orgo2 #genchem #stem #trendingtopics #womeninstem #STEMTok #science #scientist #scientistsoftiktok

Replying to @Samaria I got y’all! Follow me on those platforms @genchemwithdrj. #genchemwithdrj #generalchemistry #Genchem #chemistry

Replying to @Samaria I got y’all! Follow me on those platforms @genchemwithdrj. #genchemwithdrj #generalchemistry #Genchem #chemistry

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