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General Chemistry > Chapter 1 > Flashcards

Chapter 1 Flashcards

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1
Q

Mass number

A

Sum of protons and neutrons in a nucleus

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2
Q

How do you find the number of electrons?

A

Electrons equal the number of protons when the atom is neutral and vary when the atom is positively or negatively charged

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3
Q

How do you find the number of protons ?

A

Equal to the atomic number

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4
Q

How do you find the number of neutrons ?

A

Atomic mass - atomic number = number of neutrons

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5
Q

Which subatomic particle is most important for determining isotopes ?

A

Neutrons

Varying number of neutrons allow for different masses of an atom to exist even though the atomic number stays the same

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6
Q

Atomic mass

A

Sum of the mass of protons and neutrons in a given atom

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7
Q

Atomic weight

A

Weighted average of naturally occurring isotopes of an element

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8
Q

What was Planck’s first quantum theory ?

A

Energy emitted as electromagnetic radiation from matter comes in discrete bundles called quanta

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9
Q

Planck’s relation formula

A

E=hf

H is Planck’s constant = 6.626x10^-34 js
F is the frequency of radiation
E is the energy emitted

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10
Q

Formula for angular momentum of an electron orbiting a hydrogen nucleus

A

L= nh/2pi

N is the principal quantum number, positive integer
H is Planck’s constant

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11
Q

Energy of electron equation

A

E = -Rh/n^2

Rh= 2.18x10^-18 J/ electron

The energy of electron increases as the electron gets farther from the nucleus because the energy becomes LESS NEGATIVE

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12
Q

Ground state

A

Elections are in lowest orbital

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13
Q

Excited state

A

At least one electrons moved to a sub shell

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14
Q

Electromagnetic energy of photons can be determined by

A

E= hc/ lambda=-Rh[1/ni^2-1/nf^2]

C - speed of light in vacuum ( 3.0x10^8m/s)
Lambda is the wavelength of radiation

This is the energy emitted by the photon as an electron returns from the excited state back to its ground state

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15
Q

Lyman series

A

Hydrogen emission lines starting from n =1

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16
Q

Balmar series

A

H emission lines starting from n =2

17
Q

Paschen series

A

H emission lines starting from n=3

18
Q

What happens as en electron goes from higher energy level to a lower one ?

A

AHED

A-absorbs light
H- higher energy
E- excited
D- distant from nucleus

19
Q

What does a positive E correspond to ? Negative E ?

A 
\+E = emission 
-E = absorption
20
Q

Heisenberg uncertainty principle

A

It is impossible to determine the exact location of electron

21
Q

Pauli’s exclusion principle

A

No two electrons can have the same 4 quantum numbers

22
Q

N - first principle quantum number

A

Any positive integer value
Higher value of n denotes higher energy level
Maximum number of electrons within a shell is 2n^2
Difference in energy between two shells decreases as the distance increases

23
Q

L - angular momentum

A

Refers to shape and number of subshells
N-1 limits the number of subshells
S,p,d,f
Maximum number of subshells is 4l+2

24
Q

Magnetic quantum number (ml)

A

S-l is 1
P-l is 0,-1,1
D-l is 0,-1,1,-2,2
F-l is 0,-1,-2,-3,1,2,3

25
Q

Ms - spin quantum number

A

An object spinning about its axis
+ 1/2-
-1/2

26
Q

Paired spins

A

When two electrons in the same orbitals have opposite spins

27
Q

Parallel spins

A

Electrons in different orbitals with the same ms value have parallel spins

28
Q

Building up principle (aufbau principle )

A

Electrons fill from lower to higher energy

29
Q

What is the order of electron configuration ?

A 
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d
7s 7p
30
Q

How do you wrote the electron configuration for positively charged atoms ?

A
  • remove electrons from subshell of highest n value

- if multiple subshells are tied to highest n value , use highest l value

31
Q

Paramagnetic

A

Materials composed of atoms with unpaired electrons will orient their spin to align with the magnetic field and will be attracted to the magnetic field

32
Q

Diamagnetic

A

Materials that have atoms that have paired electrons and so they are slightly repelled by the magnetic field

33
Q

Valence electron rules

A

Groups 1 to 2- only the highest s subshell electrons are the valence electrons

Groups 3 to 12 - electrons are highest in s and d

Groups 13 to 18 - electrons are highest in s and p

Lanthanides and actinides - valence electrons are those in highest f and s shells

General Chemistry (5 decks)

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