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Ardından atomun sembolünün nasıl okunacağı, kütle numarası, atom numarası, çekirdek yükü, iyon yükü ve elektron sayısı gibi kavramlar detaylı şekilde açıklanıyor. Eğitimci, bu kavramları örneklerle pekiştiriyor ve magnezyum atomu üzerinden hesaplamalar yaparak konuyu somutlaştırıyor. Video, öğrencilere sınavlarda karşılaşabilecekleri soru tiplerini göstererek ve konuyu iyi çalışmanın önemini vurgulayarak sonlanıyor."]},"endTime":581,"title":"TYT Kimya: Atomun Yapısı Dersi","beginTime":0}],"fullResult":[{"index":0,"title":"Atomun Yapısı","list":{"type":"unordered","items":["Atom, bir elementin fiziksel ve kimyasal özelliklerini taşıyan en küçük taneciktir.","Atomu oluşturan temel tanecikler proton (artı yüklü), elektron (eksi yüklü) ve nötron (yüksüz) olup, bunları bilmemiz gerekmektedir."]},"beginTime":19,"endTime":50,"href":"/video/preview/12743843548880504235?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=19&ask_summarization=1"},{"index":1,"title":"Atomun Gösterimi","list":{"type":"unordered","items":["Bir X atomunun sol üst köşesindeki değer kütle numarasını (A), sol tarafındaki değer nötron sayısını (N), sol alt köşesindeki değer proton sayısını (Z) ifade eder.","Sağ üst köşedeki değer iyonun yükünü (eksi veya artı) ifade eder, sağ alt köşedeki değer ise elektron sayısını gösterir.","Proton sayısı aynı zamanda atom numarası ve çekirdek yükü olarak da ifade edilebilir."]},"beginTime":50,"endTime":191,"href":"/video/preview/12743843548880504235?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=50&ask_summarization=1"},{"index":2,"title":"Kütle Numarası ve İyonlar","list":{"type":"unordered","items":["Kütle numarası (A) aynı zamanda nükleon sayısı olarak da bilinir ve proton sayısı ile nötron sayısının toplamına eşittir (A = Z + N).","Eksi yüklü iyonlar elektron almış, artı yüklü iyonlar elektron vermiş atomlardır; eksi yüklü iyonlara anion, artı yüklü iyonlara katyon denir.","İyon yükü, proton sayısı ile elektron sayısı arasındaki farktır (İyon yükü = Proton sayısı - Elektron sayısı)."]},"beginTime":191,"endTime":431,"href":"/video/preview/12743843548880504235?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=191&ask_summarization=1"},{"index":3,"title":"Magnezyum Örneği","list":{"type":"unordered","items":["Magnezyum atomunun kütle numarası 24, nötron sayısı 12, proton sayısı 12 ve iyon yükü +2'dir.","Kütle numarası, proton ve nötron sayısının toplamına eşittir (24 = 12 + 12).","İyon yükü, proton sayısı ile elektron sayısı arasındaki farktır; proton sayısı, iyon yükü ile elektron sayısının toplamına eşittir."]},"beginTime":431,"endTime":509,"href":"/video/preview/12743843548880504235?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=431&ask_summarization=1"},{"index":4,"title":"Öneriler","list":{"type":"unordered","items":["Atomun yapısı konusu TYT sınavında önemli bir konudur ve halledilebilir sorulardır.","Atom ve periyodik sistem konusunu iyi çalışıp, Milli Eğitim Bakanlığı kitabındaki ve soru bankalarındaki soruları çözmek önemlidir."]},"beginTime":509,"endTime":559,"href":"/video/preview/12743843548880504235?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=509&ask_summarization=1"}],"linkTemplate":"/video/preview/12743843548880504235?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=%%timestamp%%&ask_summarization=1"},"isAdultDoc":false,"relatedParams":{"text":"Tyt 2023 kimya - atomdaki temel tanecikleri hesaplama","related_orig_text":"Atomus Simplifies","related_porno":false,"related_less_3m_off":true,"client":"d2d","no_cnt":1,"related_src":"serp","related":"{\"porno\":false,\"vfp\":1,\"orig_text\":\"Atomus 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Kaynak👉345 AYT Fizik SORU Bankasi + Aydin Yayinlari AYT DERS Isleyiş Modülü https://www.ucdortbes.com/ayt-fizik-s... https://www.aydinyayinlari.com.tr/fiz... 👉İzlemeden Sakin Sinava...","preview":{"posterSrc":"//avatars.mds.yandex.net/get-vthumb/3699080/2e1cdf09f3aaac540b4c91089e3bdb71/564x318_1","videoSrc":"https://video-preview.s3.yandex.net/R_5xIQIAAAA.mp4","videoType":"video/mp4"},"target":"_self","position":"9","reqid":"1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL","summary":{"isFull":true,"fullTextUrl":"/video/result?ask_summarization=1&numdoc=1&noreask=1&nomisspell=1&parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=videoid:11387386755529633540","teaser":[{"list":{"type":"unordered","items":["Bu video, bir öğretmenin atom fiziği konusunu anlattığı kapsamlı bir eğitim dersidir.","Video, atom fiziğinin temel konularını sistematik bir şekilde ele almaktadır. İlk olarak atom modelleri (Milikan, Thompson, Rutherford ve Bor) anlatılmakta, ardından elektronların yörüngelerindeki enerji ilişkileri, yörünge numarası (n) ile toplam enerji arasındaki ilişki, ışıma ve kendiliğinden emisyon olayları detaylandırılmaktadır. Son bölümde ise hidrojen atomunun enerji seviyeleri, ışıma süreçleri ve elektromanyetik dalgalarla ilgili soru çözümleri yapılmaktadır.","Videoda elektronların yörüngelerindeki enerji ilişkileri (E = -Rz/n² formülü), ışıma sayısının formülü (n(n-1)/2), fotonun enerjisinin hesaplanması, kesikli değerler kavramı ve dalga boyu-enerji ilişkisi gibi önemli fizik formülleri ve kavramlar formüllerle ve örneklerle açıklanmaktadır. Ayrıca, n'nin artmasıyla birlikte elektronun yörüngeden kopma eğiliminin arttığı ve bunun kimyasal anlamının üst yörüngelerden elektron koparmak daha kolay olduğu vurgulanmaktadır."]},"endTime":1948,"title":"Atom Fiziği Eğitim Dersi","beginTime":0}],"fullResult":[{"index":0,"title":"Atom Fiziğiye Giriş","list":{"type":"unordered","items":["Atom fiziğine giriş olarak atom modelleri, atomun ışımalari, uyarılma düzeyleri ve hidrojen atomunun spektrumu konuları ele alınacak.","Milikan'ın yağ damlası deneyi ile elektronun yük miktarı ve kütlesi ilk defa ölçülmüştür."]},"beginTime":0,"endTime":63,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=0&ask_summarization=1"},{"index":1,"title":"Atom Modelleri","list":{"type":"unordered","items":["Thompson atom modelinde atom bir üzümlü keke benzetilmiş, atomun yükçe nötr olduğu ve artı ve eksilerin içinde rastgele dağıldığı belirtilmiştir.","Rutherford atom modelinde ilk defa atomun çekirdeği kavramı ortaya atılmış, elektronların merkezde artı yüklü çekirdeğin etrafında rastgele ivmeli hareket ettiği düşünülmüştür.","Rutherford modelindeki asrın hatası, elektronların rastgele ivmeli hareket yapsalar dışarıya foton salarak enerjisi azalıp çekirdeğe düşmesi gerektiği fikrine dayanmaktadır."]},"beginTime":63,"endTime":227,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=63&ask_summarization=1"},{"index":2,"title":"Bor Atom Modeli","list":{"type":"unordered","items":["Bor atom modelinde Rutherford'un çekirdek kavramı doğrulanmış, ancak elektronların çekirdeğin etrafında rastgele değil belirli yörüngelerde dolanması öne sürülmüştür.","Bor modelinde ilk defa yörünge kavramı ortaya atılmış, elektronların belirli yörüngelerde dolanırken sahip oldukları toplam enerji, açısal momentum ve yörünge yarıçapları vardır."]},"beginTime":227,"endTime":283,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=227&ask_summarization=1"},{"index":3,"title":"Atom Enerjisi Formülü","list":{"type":"unordered","items":["Atom enerjisi formülü E = -r × z²/n²'dir; burada r Readberg sabiti, z atom numarası, n ise yörünge numarasıdır.","Atom numarası arttıkça toplam enerji artar, ancak başındaki eksi işaretinden dolayı toplam enerji azalır.","Hidrojen atomunda atom numarası sabittir (z=1), bu nedenle yörünge numarası (n) arttıkça toplam enerji artar."]},"beginTime":296,"endTime":391,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=296&ask_summarization=1"},{"index":4,"title":"Yörünge Değişimi ve Enerji İlişkisi","list":{"type":"unordered","items":["Yörünge numarası (n) ile toplam enerji doğru orantılıdır; yani yörünge numarası arttıkça toplam enerji artar.","Üst yörüngeye geçiş yapan atomlar toplam enerjileri arttığı için iyonlaşmaya (kopmaya) daha yakınlaşır.","Son yörünge elektronlarını koparmak daha kolaydır çünkü toplam enerjileri daha büyüktür."]},"beginTime":391,"endTime":438,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=391&ask_summarization=1"},{"index":5,"title":"Bağlanma Enerjisi","list":{"type":"unordered","items":["Bağlanma enerjisi, toplam enerjinin eksilisidir ve E = -Etoplam formülüyle hesaplanır.","Yörünge numarası (n) arttıkça toplam enerji artar, ancak bağlanma enerjisi azalır.","Elektron yörünge numarası arttıkça kopmaya yakınlaşır, bu nedenle onu koparmak için daha az enerji gerekir."]},"beginTime":438,"endTime":546,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=438&ask_summarization=1"},{"index":6,"title":"Yörünge Yarıçapı","list":{"type":"unordered","items":["Yörünge yarıçapı formülü R = a × n²/z'dir; burada a Bor sabiti, z atom numarası, n yörünge numarasıdır.","Yörünge numarası (n) ile yörünge yarıçapı doğru orantılıdır ve n² ile artar.","Yörünge numarası arttıkça elektriksel kuvvet azalır, bu nedenle elektron kopmaya daha yakınlaşır."]},"beginTime":546,"endTime":677,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=546&ask_summarization=1"},{"index":7,"title":"Açısal Momentum ve Diğer Özellikler","list":{"type":"unordered","items":["Elektronun açısal momentumu formülü L = n × h/2π'dir; burada n yörünge numarası, h Planck sabiti, 2π ise paydadır.","Yörünge numarası (n) arttıkça açısal momentum, yörünge yarıçapı ve toplam enerji artar.","Yörünge numarası arttıkça çizgisel hız, kinetik enerji, açısal hız azalır ve dolanım periyodu artar."]},"beginTime":677,"endTime":885,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=677&ask_summarization=1"},{"index":8,"title":"Atomlarda Uyarılma ve Kendiliğinden Emisyon","list":{"type":"unordered","items":["Atomlar temel hal (n=1) dışında n=2, n=3 gibi uyarılma düzeylerine veya iyonlaştırılabilir (elektronun yörüngeden kopması).","Birinci uyarılma düzeyi n=2, ikinci uyarılma düzeyi n=3 olarak adlandırılır ve yörünge numarası ile uyarılma düzeyi arasında ayrım yapılmalıdır.","Uyarılan atomlar 10 üzeri eksi 8 saniye gibi kısa bir sürede kendiliğinden temel hale inmeye çalışır ve bu duruma kendiliğinden emisyon denir."]},"beginTime":889,"endTime":1016,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=889&ask_summarization=1"},{"index":9,"title":"Atomlarda ışıma ve enerji kaybı","list":{"type":"unordered","items":["Bir atom n=3'den temel hale inerken, bir basamak bir basamak inebilir veya tek seferde inebilir; ışıma sayısını bulmak için n(n-1)/2 formülü kullanılır.","Atom temel hale inerken dışarıya elektromanyetik dalga (foton) yayar ve bu fotonun enerjisi, atomun kaybettiği enerji kadardır.","Fotonun enerjisi E=hf veya E=hc/λ formüllerinden bulunur; fotonun enerjisi frekansla doğru orantılı, dalga boyuyla ters orantılıdır."]},"beginTime":1016,"endTime":1416,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=1016&ask_summarization=1"},{"index":10,"title":"Bor Atom Modelinde Kesikli Değişkenler","list":{"type":"unordered","items":["Bor atom modeline göre enerji, açısal momentum ve elektronların yörünge yarıçapı kesiklidir (belirli değerleri alır).","Enerji formülü E=-RZ²/n², açısal momentum formülü L=nh/2π ve yörünge yarıçapı formülü r=a×n²/Z'dir.","Bu değerler n (yörünge numarası) değiştiğinde değiştiği için kesikli (quantumlu) olarak adlandırılır."]},"beginTime":1416,"endTime":1519,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=1416&ask_summarization=1"},{"index":11,"title":"Enerji ve Işıma Hesaplamaları","list":{"type":"unordered","items":["Bir sistemin kaybettiği enerji dışarıya ışınılır ve bu enerji hesaplanabilir.","Frekans enerji ile doğru orantılı, dalga boyu ise enerji ile ters orantılıdır.","Enerji sıralaması yapılarak ışınaların frekans ve dalga boyu sıralamaları belirlenebilir."]},"beginTime":1526,"endTime":1616,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=1526&ask_summarization=1"},{"index":12,"title":"Hidrojen Atomu Işıma Sorusu","list":{"type":"unordered","items":["Hidrojen atomunun enerji formülü E = -R × Z²/n² şeklindedir.","X, Y ve Z ışınalarının arada kaybettiği enerjiler hesaplanarak sıralanabilir.","Elektromanyetik dalgalarda çizgisel momentum enerji ile doğru orantılıdır ve boşlukta hızları eşittir."]},"beginTime":1616,"endTime":1830,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=1616&ask_summarization=1"},{"index":13,"title":"Atomik Hareketler ve Yüzyönler","list":{"type":"unordered","items":["Çekirdeğin atom numarası elektronun yörünge hızını etkiler.","Elektron çekirdekten uzaklaşarak yeni bir kararlı yörüngeye geçerse hızı azalır.","Elektronun açısal momentumu artarsa hızı azalır çünkü açısal momentum n × h/2π formülüyle ilgilidir."]},"beginTime":1830,"endTime":1893,"href":"/video/preview/11387386755529633540?parent-reqid=1769622592263939-9810631034900139284-balancer-l7leveler-kubr-yp-sas-67-BAL&text=Atomus+Simplifies&t=1830&ask_summarization=1"},{"index":14,"title":"Uyarılma Düzeyi ve Işıma","list":{"type":"unordered","items":["Temel halde bulunan bir hidrojen atomu üç uyarılma düzeyine kadar uyarılabilir.","n=4'ten temel hale dönerken en az bir, en fazla altı farklı ışıma yapılabilir.","Derste elektromanyetik ışıma ve atomik hareketler konuları 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