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MED109 > WEEK1-2 > Flashcards

WEEK1-2 Flashcards

1
Q

What is an Atom?

A

an atom is the smallest unit of an element that retains the chemical properties of that element

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2
Q

How many distinct regions does an atom have?

A

Atom has two distinct regions: 1. dense positively charged nucleus 2. surrounding the nucleus is a diffuse region of negative charge populated by electrons.

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3
Q

How small is an electron compared to a proton or neutron?

A

Nearly two thousand times smaller.

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4
Q

What are isotopes?

A

Isotopes are atoms of the same element that differ in the number of neutrons

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5
Q

How do you write the isotopic notation?

A

List the number of protons neutrons and electrons

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6
Q

what are ions?

A

charged species formed from a neutral atom or molecule when electrons are gained or lost

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7
Q

what is a cation?

A

positively charged ion

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8
Q

what is an anion?

A

Negatively charged Ion

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9
Q

what is the formula for determining Atomic mass from isotopes?

A

Atomic mass=(mass1)(abundance%1) + (mass2)(abundance%2)

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10
Q

What is electronegativity? describe its trend on the periodic table.

A

Electronegativity is the degree of attraction an atom has for electrons. It is an atoms ability to attract and bind with electrons. It increases to the right of the periodic table and up.

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11
Q

What is Atomic Radius? Describe its trend on the periodic table.

A

Atomic radius is the distance between the center of a nucleus and the outermost shell of an atom. It decreases from left to right on the periodic table and top to bottom.

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12
Q

What is ionization energy? Describe its trend on the periodic table.

A

Ionization energy is the minimum amount of energy required to remove an electron from an isolated atom or molecule. Ionization energy increases to the right of the periodic table and up.

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13
Q

What is electron affinity? what is its trend on the periodic table?

A

electron affinity is the ability of an atom to gain an electron. It increases to the right of the periodic table and up.

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14
Q

Who invented the periodic table?

A

Dmitri Mendeleev invented the periodic table in 1869

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15
Q

What is the periodic law?

A

Elements are arranged in order of increasing atomic number

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16
Q

How large is an atom compared to its nucleus?

A

Approximately 100,000 times larger

17
Q

In order for chemists to understand the chemical properties of elements they needed to understand what?

A
  • the nature of electrons
  • their behavior
  • the space where they move around the nucleus
18
Q

What is the Photo-electric effect?

A

Photo electric effect is when light shinning on a metal surface causes it to emit electrons

19
Q

Who was Einsteins work on photoelectric effect influenced by?

A

Max Planks idea of quantized energy

20
Q

Describe the first Quantum number.

A

The Principle quantum number(n): Describes the distance of the orbital from the nucleus, its size and its energy. As n increases, so does the size, distance and energy. Also known as shell

21
Q

Describe Bhor model of the atom.

A

Bohr described the atom as electrons found in definite orbits surrounding the nucleus. Like planets orbiting the sun.

22
Q

What is an orbital?

A

Regions of high probability to find the electrons

23
Q

State the Heisenberg Principle

A

the accurate knowledge of the position and movement of electrons is impossible

24
Q

Describe the second quantum number

A

Angular Momentum quantum number(l). Tells the shape of an orbital (represented by s,p,d,f). AKA sub-shell

25
Q

Describe the third quantum number

A

Magnetic Quantum Number(m1): specifies the orientation in space of an orbital. It divides the sub-shell into individual orbitals which hold electrons

26
Q

Describe the fourth quantum number?

A

Magnetic spin

27
Q

How many orbitals does sub-shell s have?

A

1
l=0,m1=0

28
Q

How many orbitals does sub-shell p have?

A

3
l=1, m1=-1,0,1

29
Q

How many orbitals does sub-shell d have?

A

5
l=2, m1=-2,-1,0,1,2,

30
Q

How many orbitals does sub-shell f have?

A

7
l=3
m1=-3,-2,-1,0,1,2,3

31
Q

what is atomic number?

A

Number of protons

32
Q

what is mass number?

A

Number of protons + neutrons

33
Q

what is atomic mass?

A

average mass of isotopes of a naturally occurring element

34
Q

what does iso-energetic mean ?

A

orbitals with the same value of n and l but different value of m1
2px=2py=2pz

MED109 (5 decks)

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