Chapter 5 atomic theory/structure Flashcards

1
Q

All elements have neutrons, except what?

A

The simplest of hydrogen Dash not an isotope

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2
Q

Isotopes are what?

A

Isotope means same place.

Atoms of the same element with different numbers of
neutrons (which means a different atomic mass)

They belong in the same place on the periodic table

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3
Q

Summarize the atomic theory by Dalton

A

Elements are composed of indivisible particles called atoms

Atoms of the same element are chemically alike. Atoms of different elements are chemically different.

Atoms combine in simple WHOLE NUMBER RATIOS to form compounds

Atoms of the same two elements can combine in more than one way to form different compounds

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4
Q

What part of Dalton’s at atomic theory has been discarded based on evidence

A

We now know:
Adams are composed of subatomic particles

Not all atoms of a specific element have the same mass

Adams under special circumstances can be decomposed

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5
Q

What is the law of definite composition

A

A compound always contains two or more elements, chemically combined in a definite proportion to mass

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6
Q

What is the law of multiple proportions?

A

Adams of two or more elements make combine in different ratios to produce more than one compound

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7
Q

Force equals what?

A

Distance of charges to each other, and the amount of charge

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8
Q

What are charged particles called?

A

Ions

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9
Q

What did faraday discover ?
1791 through 1867

A

Some substances can conduct electricity, when dissolved in water, some compounds can decompose into charged particles that then move based on attraction for other charged particles-ions

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10
Q

JJ Thompson discovered the electron using experiments using cathode rays. What else did he discover about electrons?

A

 He discovered electrons:
travel in straight lines
are negative in charge
deflected by electricity and magnetic fields
Produce sharp shadows
capable of moving small paddle wheel

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11
Q

What are the symbols for subatomic particles?

A

Proton is a small p with a plus
Neutron is a small and w/ small o
Electron is small e with -

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12
Q

What is the charge for each subatomic particle?

A

Proton is positive
neutron is neutral
electron is negative

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13
Q

What is Amu stand for?

A

Atomic mass unit

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14
Q

What is the AMU of each subatomic particle?

A

Proton is one neutron is one electron is zero

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15
Q

Describe Rutherford’s gold foil experiment observations as he was messaging, the alpha particles straight through the gold foil, discovering the neucleus

A

Observation: most of the alpha particles went straight through the gold foil. conclusion most of the atom is empty Space.

Observation: very few alpha particles bounced off the gold foil.
Conclusion: the alpha particles hit some thing: small, positive, massive. NUCLEUS

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16
Q

Most of the mass of an atom is where

A

In the nucleus - protons and neutrons

17
Q

Most of the atom is formed of what

A

Empty space- electron cloud

18
Q

What is the atomic number?

A

The number of protons in the nucleus

19
Q

What is an isotope?

Not sure if this is correct?? Text og 96
Says isotope is same atomic number diff atomic mass

A

The number of atoms of the same element with different number of neutrons

20
Q

What is mass number?

A

Protons plus neutrons added together.

Priests and nuns go to mass

21
Q

Is mass number on the periodic table

A

No

22
Q

In the mass number,
what is hyphen notation?

A

After the-is the mass number
Lithium -6
Lithium -7

23
Q

What is nuclear notation?

A

6 (MASS NUMBER)
Li (Symbol)
3 (ATOMIC NUMBER)

24
Q

Explain atomic mass

A

This is the average mass of the isotopes of an element.
This is a weighted average mass of iPad isotopes with larger abundance in nature account for more of the average mass. This is NOT the same as calculating the mean of a set of numbers.

25
Q

When there’s a neutral charge, what is equal?

A

Protons and electrons

26
Q

Atoms, form ions, through loss or gain of what

A

Electrons

27
Q

107 +
47

     Ag

Explain this notation

A

107 is mass # and # of protons and neutrons

47 is # of protons

+ is charge, # of electrons

28
Q

What three numbers are always the same

A

Atomic number, protons, electrons,

29
Q
A
30
Q

When it’s a low frequency, electrons tap the metal instead of bouncing off

A
31
Q

In an isotope the number after the-equals the what?

A

Mass number

32
Q

How do we get the mass number?

A

Protons plus neutrons added together

33
Q

Is atomic mass and average mass the same?

A

Yes

34
Q

Mass number is the number of neutrons and protons in an isotope!!

A
35
Q

Average atomic mass (equation) should be somewhat the same as average mass on the periodic table!

A
36
Q

Mass # - atomic #= neutrons in isotope!!!

A
37
Q

What is the charge of a neutron?

A

study guide says

nothing or 0

38
Q

What’s the difference between an ion and an isotope?

A

Isotopes -different #neutrons.
ion gained or lost electrons, a negative or positive charge.