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Chemistry > Chem Week Two > Flashcards

Chem Week Two Flashcards

1
Q

What make atoms?

A

Sub-atomic particles. The three most common ones are neutrons, electrons, and protons. An atom is mostly empty space.

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2
Q

What is atomic mass based on?

A

Carbon-12

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3
Q

What is the atomic number equal to?

A

The number of protons in an atom.

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4
Q

1 gram in dalton (Da or u)

A

6.022 * 10^23

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5
Q

What are the properties of protons?

A

They have a positive charge (p+)

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6
Q

What are the properties of neutrons?

A

They have a neutral charge (n0)`

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7
Q

What are the properties of electrons?

A

They have a negative charge (e-)

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8
Q

What make up a nucleus?

A

Protons and neutrons. The nucleus has most of the mass of an atom and has a positive charge.

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9
Q

When the atom has a neutral charge, what is the number of protons and electrons?

A

There are an equal number of protons and neutrons.

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10
Q

What are the three groups of elements?

A
  1. Semi-metals or metalloids.
  2. Nonmetals
  3. Metals
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11
Q

What are the properties of metals?

A
  1. Are solid at room temperature (except for mercury.)
  2. Have a reflective surface.
  3. Conduct heat and electricity.
  4. Are malleable
  5. Are ductile (can be made into wires)
  6. Readily loose electrons and become cations (positively charged ions).
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12
Q

What are the properties of nonmetals?

A
  1. Found in all three states.
  2. Poor conductors of heat and electricity
  3. Solids are not malleable
  4. Readily gain electrons and become anions (negatively charged ions)
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13
Q

What are the properties of semimetals/metalloids?

A
  1. Are semi-conductors

2. Have some properties of both nonmetals and metals.

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14
Q

What are the groups of elements on the periodic table?

A
  1. Alkali metals
  2. Alkaline metals (tend to lose electrons)
    3-12. Transition metals
    Post-transition metals
  3. Halogens (negatively charged)
  4. Noble/inert gases (do not react, monatomic)
    Lanthanoids
    Actinoids
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15
Q

What is an ion?

A

An atom where the number of electrons does not equal the number of protons.

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16
Q

What is an atom with a positive charge (more protons than electrons)?

A

A cation.

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17
Q

What is an atom with a negative charge (more electrons than protons)?

A

A anion.

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18
Q

What does an atom lose or gain so that it becomes an ion?

A

Electrons. The number of protons stays the same.

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19
Q

What is a polyatomic ion?

A

A collection of ions.

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20
Q

What groups tends to form ions?

A

Nonmetals

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21
Q

What are isotopes?

A

When the number of protons does not equal the number of neutrons. The number of protons stay the same, but the number of neutrons is different.

22
Q

What are the rules for naming monatomic anions?

A

The element ending changes to -ide.

23
Q

What are the rules for naming monatomic cations.

A

The ending stays the same, and it is just called an [element] ion.

24
Q

What does an electron always try to do?

A

Lower its potential energy whenever possible. They always try to be as close to protons as possible to achieve this.

25
Q

What is a valence electron?

A

An electron that connects to another atom by the atom giving up an electron.

26
Q

Do metal valence electrons have higher energy than non metal valence orbitals?

A

Yes. Nonmetal valence orbitals want to go to lower energy.

27
Q

Name properties of nonmetal valence orbitals.

A
  1. They have room for incoming electrons.

2. They have low potential energy

28
Q

What does an encounter between a metal valence electron and a nonmetal valence orbital result in?

A

An electron transfer. An electron transfers and results in an ionic bond.

29
Q

What does an ionic bond result in?

A

It can result in a ionic compound that can result in an extended solid.

30
Q

Periodic law.

A

Elements in columns tend to react similarly as other elements in the column.

31
Q

Is it easier to take an electron from a nonmetal or a metal?

A

A metal. Metals have higher energy than non-metals, resulting in them loosing electrons easier to lower its energy.

32
Q

Electronegativity

A

The property of an atom to attract bonding electrons. This is when electrons are joining an atom (bonding or incoming.)

33
Q

What do electrons that attract bonding electrons have?

A

They have low energy orbitals (usually nonmetals) that aren’t completely filled. So, they have room for electrons from other atoms to join.

34
Q

What do nonmetals have?

A

Low energy orbitals available.

35
Q

How strong are metals in terms of electronegativity?

A

They are weakly electronegative.

36
Q

Atomic radi

A

How large the cloud of electron is in neutral elements. This is related to nuclear charge.

37
Q

1 angstrom (Å) in meters

A

10^-10 meters

38
Q

How do electrons become more attracted to the nucleus?

A

The charge increases.

39
Q

Ionization energy

A

How much energy is needed to give up an electron.

40
Q

What electrons are easiest to separate from its atom?

A

Electrons in high energy orbitals. These have small ionization energy.

41
Q

What do metals like to be?

A

Cations. They have their outermost electrons in high energy orbitals. This makes electrons easy to remove and have the atom have a small/low ionization energy.

42
Q

What do nonmetals like to be?

A

They like to gain electrons, becoming anions.

43
Q

What orbitals to nonmetals have?

A

Low energy orbitals, and therefore, have large electronegativity, making electrons harder to get rid of.

44
Q

Density equation

A

ρ = mass/vol or d=mass/vol

45
Q

Equation for energy change in a system

A

ΔE = Efinal - Einitial. When energy is flowing in, the energy is positive. When energy is flowing out, the energy is negative.

46
Q

1st law of thermodynamics

A

Conversation of energy. The equation is ΔEuniv = ΔEsystem + ΔEsurroundings OR ΔEsystem = -ΔEsurroundings

47
Q

Energy moving between a systems and its surroundings equation

A

ΔEsystem = q+w, where q = heat (can be absorbed [+] or released [-]) and w = work (work done on system [+] or done by system [-])

48
Q

ΔE

A

direction of energy flow. The direction of energy flow is from a hot area to a cold area.

49
Q

What happens when you add heat to a system?

A

The temperature increases or it goes into a phase change.

50
Q

The equation of the relationship between the amount of heat added to a given amount of the substance and the corresponding temperature increase.

A

q = CΔT OR q = msΔT, where C = heat capacity for increasing heat by 1*C, and s = specific heat capacity

Chemistry (9 decks)

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