Term
| 3. What is a line spectrum/atomic emission spectrum? How is this diffferent from the continuous spectrum? |
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Definition
| Line spectrum/atomic emission spectrum only shows certain colors or wavelengths. Continuous shows all colors and wavelengths. |
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Term
| Why is an atomic emission spectrum often called an atoms fingerprint? |
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Definition
| Each element has their own characteristic line spectra |
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Term
| Why is the Bohr model only accurate for hydrogen? |
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Definition
| Bohr couldn't predict other's wavelengths using math b/c they had more than 1 electron. |
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Term
| What is Heisenburg's uncertainty principle? How does this help show that Bohr's model isn't entirely correct? |
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Definition
| -Both position and momentum of an electron cannot be simultaneously known. This helps show that the Bohr model isn't entirely correct b/c it assumes we do know the momentum and position of an electron, but we don't so we have to use probability to estimate the electrons location. |
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Term
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Definition
| Space around the nucleus where there is a high probability of finding an electron |
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Term
| List the types of orbitals in order of increasing energy |
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Definition
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Term
| How many different types of s orbitals exist? |
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Definition
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Term
| What does an S orbital look like? |
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Definition
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Term
| What is the electron capacity of the s sublevel? Of one s orbital? |
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Definition
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Term
| How many different types of P orbitals exist? |
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Definition
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Term
| What do p orbitals look like? |
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Definition
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Term
| What is the electron capacity of the p sublevel? Of one p orbital? |
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Definition
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Term
| How many different types of d orbitals exist? |
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Definition
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Term
| What is the electron capacity of a d sublevel? Of one d orbital? |
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Definition
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Term
| Pauli exclusion principle |
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Definition
| an atomic orbital may describe at most 2 electrons |
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Term
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Definition
| electrons fill lower energy orbitals first |
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Term
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Definition
| electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible |
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