Chemistry, 02.10.2019 05:30 125712

Which would melt first, the element
germanium with a melting point of 1210 k or
the element gold with a menting point of 1064
°c? explain your answer. show your work.

Answers: 2

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Answer from: MK100

The element that would melt first is germanium

From the question,

We are to determine the element that would melt first.

The element that would first melt is the element with the lower melting point.

From the question,

The melting point of element germanium = 1210 K

and

The melting point of element gold = 1064 °C

First, we will convert the melting points to same units of temperature

Convert 1064 °C to Kelvin, K

Using the formula

K = °C + 273

∴ 1064 °C to Kelvin is

K = 1064 + 273

K = 1337

∴ 1064 °C = 1337 K

This means

The melting point of element gold = 1337 K

Now comparing the melting point of gold (1337 K) to the melting point of germanium (1210 K),

We can observe that the melting point of element germanium is lower.

Therefore, element germanium would melt first.

Hence, the element that would melt first is germanium

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Answer from: sbelgirl2000

Explanation:

First, get both values into the same units

To covert from Kelvin to degrees C, subtract 273.15

1210 - 273.15 =936.85

Melting point of germanium=936.85 degrees C

Melting point of gold= 1064 degrees C

Therefore germanium would melt first because it has the lower melting point.

Answer from: Quest

Evaporation: this is when warmth from the sun causes water from oceans, lakes, streams, ice and soils to rise into the air and turn into water vapour (gas). water vapour droplets join together to make clouds! condensation: this is when water vapour in the air cools down and turns back into liquid water.

Answer from: Quest

assuming that your periodic table has eighteen columns, you should highlight the four elements in the third column from the left of the table.

explanation

neutral atoms of elements after calcium contain d electrons. the energy of d orbitals of a particular main shell lies between the energy of the s and p orbitals of the next main shell. for example, electrons in the $3d$ have energy higher than those in the $4 s$ orbital while lower than those of the $4 p$ orbital.

by the aufbau principle, electrons fill orbitals one at a time, starting from those of the lowest energy. the $4s$ orbital is therefore filled right after $3p$ orbitals and before $3 d$ orbitals.

potassium has electron configuration $[\text{ar}] 4 s^{1}$ and calcium $[\text{ar}] 4 s^{2}$ . the s orbital of a main shell holds a maximum of two electrons. the next element would thus have the electron configuration $[\text{ar}] 4 s^{2} \; 3d^{1}$ and satisfy the requirements.

a neutral atom of the element contains three electrons on top of the most recent noble gas element. it should thus be placed in the third column of the periodic table. both scandium and yttrium would satisfy the conditions. an aufbau diagram indicates that the 4f orbital is filled before the 5d. however, it appears that exceptions exists for both lanthanum and actinium. neutral atoms of the two d-block elements also demonstrate the $ns^{2} \; (n-1) p^{1}$ and should be highlighted as well.

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Which would melt first, the element
germanium with a melting point of 1210 k or
the elem...