5.3 Flashcards

1
Q

Why can’t scientists measure the diameter of a single atom?

A

Atoms have no well-defined border

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2
Q

What do you need to figure out the size of atoms?

A

Two atoms

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3
Q

Define atomic radius

A

Half the distance between the nuclei of two atoms when they are joined in a molecule

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4
Q

Atomic radius is measured in

A

Picometers

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5
Q

Molecules that can’t be single atoms will be found in

A

Diatomic molecules

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6
Q

Elements that are only found in diatomic molecules

A
Hydrogen
Oxygen
Nitrogen
Fluorine
Chlorine
Bromine
Iodine
Everything except the first form a 7
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7
Q

Atomic radius ______ from top to bottom in a group

A

Increases

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8
Q

Atomic radius ______ from left to right across a period

A

Decreases

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9
Q

The difference in size as you go down a group is _______ than the difference as you go across a period

A

Greater

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10
Q

What are shielding electrons?

A

Inner core electrons

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11
Q

Atomic radius increases down a group because

A

The shielding effect of going down another energy level is greater than the effect of increasing protons

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12
Q

Atomic radius decreases across a period because

A

Within a period, shielding effect doesn’t change, so as the number of protons increases, the electrons are pulled closer and atomic size decreases

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13
Q

Ion

A

Atom or group of atoms that has a positive or negative charge, created by the transfer of electrons

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14
Q

Metallic elements _____ one or more electrons from highest energy level to make ______ charge ions

A

Lose

Positive

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15
Q

Cation

A

Ion with a positive charge

Decreases in size

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16
Q

Nonmetallic elements ____ one or more electrons to make _______ charge ions

A

Gain

Negative

17
Q

Anion

A

Ion with a negative charge

Increases in size

18
Q

Why do atoms form ions?

A

To become more stable like a noble gas

19
Q

Ionization energy

A

Energy required to remove an electron from an atom to make a positive ion

20
Q

Ionization energy _______ as you go down a group

A

Decreases

21
Q

Ionization energy ______ from left to right across a period

A

Increases

22
Q

1st ionization energy

A

Energy to remove first outermost electron

23
Q

How can ionization energies be used to predict charges of cations?

A

Easy to remove first electron from group 1A metal atoms=little IE
Difficult to remove second electron=big IE
Group 1A metals tend to form cations with a 1+ charge because it wants to be like a noble gas

24
Q

Why is first ionization energy of nonmetal much higher than alkali metal?

A

Number of protons increases while shielding stays constant, so it’s more difficult to remove an electron

25
Q

Ionization energy decreases down a group because

A

Increases energy level= increases size=easier to remove an electron from atom so lower ionization energy

26
Q

Ionization energy increases across a period because

A

Increases in protons/charge but no change in shielding means higher ionization energy

27
Q

Metals lose electrons and ______ in size

A

Decrease

28
Q

Nonmetals gain electrons and ______ in size

A

Increase

29
Q

Size graph in a period

A
That backwards N shape from the worksheet
First leg (low and decreasing) is cations
Last leg (high and decreasing) is anions
30
Q

Electronegativity

A

Ability of an atom to attract electrons when it’s bonded to another atom

31
Q

Electronegativity ________ down a group because

A

Decreases because bigger atoms have a harder time attracting the outermost electrons

32
Q

Electronegativity ________ across a period in

A

Increases

In representative elements

33
Q

Metals have a ___ value of Electronegativity

A

Low

34
Q

Nonmetals have a _____ value of Electronegativity except for

A

High except noble gases