JEE NEET STUDY MATERIAL

💥 QUICK REVISION 💥 🌺 MECHANICS 🌺 😍@JEE_NEET_NOTES😍

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✅Menstrual Cycle (1) Menstruation occurs in human, apes and old world monkeys. (2) Menstruation is bleeding from the uterus of adult females at intervals of one lunar month. (3) Beginning of menstruation or first menstruation is called menarche. (4) The beginning of menstruation varies. It usually occurs between 12 and 15 years. (5) The cycle of events starting from one menstruation till the next one is called Menstrual Cycle. (6) In human females, menstruation is repeated at an average interval of about 28/29 days. (7) One ovum is released (ovulation) during the middle of each menstrual cycle. (8) It is regulated by certain hormones, some of which are secreted by the pituitary gland. (9) The pituitary gland is stimulated by releasing factors produced in the hypothalamus. (10) The hormones produced by the pituitary gland influence the ovaries. The hormones secreted by the ovaries affect the walls of the uterus. Phases of Menstrual Cycle The menstrual cycle consists of following four phases: (1) Menstrual Phase: (i) In a 28 days menstrual cycle,the menses takes place on cycle days 3-5. (ii) The production of LH from the anterior lobe of the pituitary gland is reduced. (iii) The withdrawal of this hormone causes degeneration of the corpus luteum and, therefore progestrone production is reduced. (iv) Production of oestrogen is also reduced in this phase. (v) The endometrium of uterus breaks down & menstruation begins. (vi) The cells of endometrium secretions, blood & unfertilised ovum constitutes the menstrual flow. (2) Follicular Phase: (i) This phase usually includes cycle days 6-13 or 14 in a 28 days cycle. (ii) The follicle stimulating hormone (FSH) secreted by the anterior lobe of the pituitary gland stimulates the ovarian follicle to secrete oestrogens. (iii) Oestrogen stimulates the proliferation of the endometrium of the uterine wall. (iv) The endometrium becomes thicker by rapid cell multiplication and this is accompanied by an increase in uterine glands & blood vessels. 🔷 Various Events during a Menstrual Cycle (3) Ovulatory Phase: (i) Both LH & FSH attain a peak level in the middle of cycle (about 14th day). (ii) Oestrogen concentration in blood increases. (iii) Rapid secretion of LH induces rupturing of graffian follicle and thereby the release of ovum. (iv) In fact LH causes ovulation. (4) Luteal Phase: (i) Includes cycle days 15 to 28. (ii) Corpus luteum secretes progestrone. (iii) Endometrium thickens. (iv) Uterine glands become secretory. ☑️Hormonal Control of MC (i) FSH stimulates the ovarian follicles to produce oestrogens. (ii) LH stimulates corpus luteum to secrete progestrone. (iii) Menstrual phase is caused by the increased production of oestrogens. (iv) LH causes ovulation (v) Proliferative phase is caused by the increased production of oestrogens. (vi) Secretory phase is caused by increased production of progestrone. 🅂🄷🄰🅁🄴 🅆🄸🅃🄷 🅈🄾🅄🅁 🄵🅁🄸🄴🄽🄳🅂 🤝🤝🤝 ▭▬▭▬▭▬▭▬▭▬▭▬▭▬ ♥️𝐅𝐎𝐑 𝐌𝐎𝐑𝐄 𝐂𝐎𝐍𝐓𝐄𝐍𝐓♥️ 💙💛𝐉𝐎𝐈𝐍💛💙 @JEE_NEET_NOTES

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ѕoмe вaѕιc concepтѕ repreѕenтed вy👉💞 What is the difference between s-block and p-block elements?🤔 ᑕOᑎᑕƐᑭTS : They are grouped as s-block or p-block according to the position of valence electrons in orbitals. The main difference between s and p block elements is that the valence electrons of the s-block elements are in the s-orbital whereas the valence electrons of the p-block elements are in the p-orbital. What behaviour of the third period of p-block elements?🤔 ᑕOᑎᑕƐᑭTS : The third period elements of p-groups with the electronic configuration 3s2 ,3pn have the vacant 3d orbitals lying between the 3p and the 4s levels of energy. Using these d-orbitals the third period elements can expand their co-valence above four. How does the presence of d-orbitals affect the properties of heavier metals?🤔 ᑕOᑎᑕƐᑭTS : The presence of d-orbitals influences the chemistry of the heavier elements in these ways: 1. The combined effect of size and availability of d orbitals considerably influences the ability of these elements to form ππ bonds. 2. The first member of a group differs from the heavier members in its ability to form pπ−pπpπ-pπ multiple bonds to itself. Why heavier metals show reluctance for pπ-pπ bonding ?🤔 ᑕOᑎᑕƐᑭTS : The heavier elements do form ππ bond but this involves d orbitals (dπ−pπ or dπ−dπ)(dπ-pπ or dπ-dπ) type bonding as the d orbitals are of higher energy than the p orbitals, they contribute less to the overall stability of molecules than does pπ−pπpπ-pπ bonding of the second row elements. What are the properties of the Boron group of elements?🤔 ᑕOᑎᑕƐᑭTS : 1. Boron is a typical non-metal, aluminium is a metal but shows many chemical similarities to boron, and gallium, indium, thallium and nihonium are almost exclusively metallic in character. 2. Boron is a fairly rare element, mainly occurs as orthoboric acid, (H3BO3), borax, Na2B4O7·10H2O, and kernite, Na2B4O7·4H2O  3. The abundance of boron in earth crust is less than 0.0001% by mass. 🅂🄷🄰🅁🄴 🅆🄸🅃🄷 🅈🄾🅄🅁 🄵🅁🄸🄴🄽🄳🅂 🤝🤝🤝 ▭▬▭▬▭▬▭▬▭▬▭▬▭▬ ♥️𝐅𝐎𝐑 𝐌𝐎𝐑𝐄 𝐂𝐎𝐍𝐓𝐄𝐍𝐓♥️ 💙💛 𝐉𝐎𝐈𝐍 💛💙 ​╔════════════════╗ ▒☞@JEE_NEET_NOTES❤️ ╚════════════════╝

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✅Notes on s-Block Elements: Covalent Character:. Small cation and large anion favors covalency. Order: LiCl > NaCl > KCl > RbCl > CsCl & . LiI > LiBr > LiCl > LiF Greater the charge on the cation greater is its polarizing power and hence larger is the covalent character: Na+CI- < Mg+2CI2 < AI+3 CI3 Greater the charge on the anion, more easily it gets polarized thereby imparting more covalent character to the compound formed eg covalent character increase in the order. NaCI < Na2SO4 < Na3PO4 c) Lattice Energies: Amount of energy required to separate one mole of solid ionic compound into its gaseous ions. Greater the lattice energy, higher is the melting point of the alkali metals halide and lower is its solubility in water d) Hydration Energy: Amount of energy released when one mole of gaseous ions combine with water to form hydrated ions. M+ (g) + aq → M+ (aq) + hydration energy X- (g) + aq → X- (aq) + hydration energy Higher the hydration energy of the ions greater is the solubility of the compound in water. The solubility of the most of alkali metal halides except those of fluorides decreases on descending the group since the decrease in hydration energy is more than the corresponding decrease in the lattice energy. Due to high hydration energy of Li+ ion, Lithium halides are soluble in water except LiF which is sparingly soluble due to its high lattice energy. For the same alkali metal the melting point decreases in the order fluoride > chloride > bromide > iodide For the same halide ion, the melting point of lithium halides are lower than those of the corresponding sodium halides and thereafter they decrease as we move down the group from Na to Cs. The low melting point of LiCl (887 K) as compared to NaCl is probably because LiCl is covalent in nature and NaCl is ionic. Anomalous Behavior of Lithium and diagonal relationship with Magnesium: Li has anomalous properties due to Very small size High polarizing Power Lithium show diagonal relationship with magnesium because both elements have almost same polarizing power. The melting point and boiling point of lithium are comparatively high. Lithium is much harder than the other alkali metals. Magnesium is also hard metal. Lithium reacts with oxygen least readily to form normal oxide whereas other alkali metals form peroxides and superoxides. LiOH like Mg (OH)2 is weak base. Hydroxides of other alkali metals are strong bases. Due to their appreciable covalent nature, the halides and alkyls of lithum and magnesium are soluble in organic solvents. Unlike elements of group 1 but like magnesium. Lithium forms nitride with nitrogen.6Li + N2 → 2Li3N LiCl is deliquescent and crystallizes as a hydrate, LiCI2H2O. Other alkali metals do not form hydrates. also forms hydrate, MgCI2.8H2O . Unlike other alkali metals lithium reacts directly with carbon to form an ionic carbide. Magnesium also forms a similar carbide. The carbonates, hydroxides and nitrates of lithium as well as magnesium decompose on heating. Li2CO3 → Li2O + CO2 MgCO3 → MgO + CO2 2LiOH → Li2O + H2O Mg (OH)2 → MgO + H2O 4LiNO3 → 2Li2O + 4NO2 + O2 2Mg ( NO3)2 → 2Mg + 4NO2 +O2 The corresponding salts of other alkali metals are stable towards heat. Lithium nitrate, on heating, decomposes to give lithium oxide, Li2O whereas other alkali metals nitrate decomposes to give the corresponding nitrite. 4LiNO3 → 2Li2O + 4NO2 + O2 2NaNO3 → 2NaNO2 + O2 2KNO3 → 2KNO2 + O2 Li2CO3, LiOH, LiF and Li3PO4 are the only alkali metal salts which are insoluble in water. The corresponding magnesium compounds are also insoluble in water. Hydrogen carbonates of both lithium and magnesium can not be isolated in solid state. Hydrogen carbonates of other alkali metals can be isolated in solid state. Sodium Hydroxide (NaOH): NaOH is stable towards heat but is reduced to metal when heated with carbon 2NaOH + 2C → 2Na +2CO + H2 FeCl3 + 3NaOH →Fe(OH)3 + 3NaCl NH4Cl + NaOH → NaCl + NH3 (pungent smell) + H2O @JEE_NEET_NOTES @JEE_NEET_NOTES

💥 FINGERTIP NOTES 💥 😍TRANSPORT IN PLANTS😍 🤪@JEE_NEET_NOTES🤪 💗@JEE_NEET_NOTES💗 🦋@JEE_NEET_NOTES🦋

💥 FINGERTIP NOTES 💥 😍 PROBABILITY 😍 🤪@JEE_NEET_NOTES🤪 💗@JEE_NEET_NOTES💗 🦋@JEE_NEET_NOTES🦋