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Ad libitum [116K]
4 years ago
15

Rutherford and his colleagues fired a beam of small, positively charged alpha particles at thin gold foil. Some of these alpha p

articles were deflected at angles as they passed through the foil.
What conclusion did Rutherford and his colleagues draw from their results?
A) The atom must contain some neutral charge spread throughout the atom. He called these particles neutrons.
B) The atom must contain some centrally located negative charge. He called this core of negative charge the nucleus.
C) The atom must contain some centrally located positive charge. He called this core of positive charge the nucleus.
D) Thomson's plum pudding model of the atom was correct. The atom contains positive charge spread throughout its structure.
Chemistry
1 answer:
Darina [25.2K]4 years ago
5 0

Answer:

C

Explanation:

The questions states that some particles were deflected meaning both the nucleus and the particles were the same charge because they repelled. Using common knowledge, we know that the nucleus is positively charged. Using this information, you can immediately eliminate choices A and B. Choice D says that the positive charge was spread throughout its structure. This is false because protons and neutrons are only found in the nucleus. Electrons are the subatomic particles found outside the nucleus, thus you can get rid of choice D, only leaving you with choice C.

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<span>The answer is
101.1032 g/mol</span>
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What is the energy of a photon with:<br> a wavelength of 827 nm? What type of radiation is it?
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Explanation:

Given parameters:

 Wavelength of photon  = 827nm  = 827  x 10⁻⁹m

Unknown:

Energy of the photon = ?

Type of radiation = ?

Solution:

The energy of a photon can be derived using the expression below:

      E = \frac{h c}{wavelength}

h is the Planck's constant = 6.63 x 10⁻³⁴m²kg/s

c is the speed of light = 3 x 10⁸m/s

Insert the parameters and solve;

      E  = \frac{6.63 x 10^{-34} x 3 x 10^{8}  }{827x 10^{-9} }  

       E = 2.4 x 10⁻¹⁹J

Type of radiation:

Near infrared radiation

 

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3 years ago
Which product has a bitter taste, is slippery when mixed with water, and can damage skin and eyes?
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How many molecules are in 0.55 moles of Cu(NO3)2?
xeze [42]
<h3>Answer:</h3>

3.3 × 10²³ molecules Cu(NO₃)₂

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right<u> </u>

<u>Chemistry</u>

<u>Atomic Structure</u>

  • Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<u>Stoichiometry</u>

  • Using Dimensional Analysis
<h3>Explanation:</h3>

<u>Step 1: Define</u>

0.55 mol Cu(NO₃)₂

<u>Step 2: Identify Conversions</u>

Avogadro's Number

<u>Step 3: Convert</u>

  1. [DA] Set up:                                                                                                     \displaystyle 0.55 \ mol \ Cu(NO_3)_2(\frac{6.022 \cdot 10^{23} \ molecules \ Cu(NO_3)_2}{1 \ mol \ Cu(NO_3)_2})
  2. [DA] Multiply/Divide [Cancel out units]:                                                         \displaystyle 3.3121 \cdot 10^{23} \ molecules \ Cu(NO_3)_2

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 2 sig figs.</em>

3.3121 × 10²³ molecules Cu(NO₃)₂ ≈ 3.3 × 10²³ molecules Cu(NO₃)₂

4 0
3 years ago
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