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Chemistry exam 1 Exam Study Guide Solutions
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Chemistry exam 1 Exam Study Guide Solutions ionic compound properties - ANSWER-- have a high melting and boiling point - they're solid at room temperature - are hard, but brittle, so they're not malleable or ductile - don't conduct electricity in solid state - are good conductors of electrici...

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  • November 11, 2024
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  • 2024/2025
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Chemistry exam 1 Exam Study Guide
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ionic compound properties - ANSWER✔✔-- have a high melting and boiling point


- they're solid at room temperature


- are hard, but brittle, so they're not malleable or ductile


- don't conduct electricity in solid state


- are good conductors of electricity in liquid state or when dissolved in water


- they vary from very soluble to insoluble in water, they're not soluble in non-polar

solvents (oil)


define ionic compounds - ANSWER✔✔-made by the chemical combination of metallic

and non-metallic elements


nanoscience - ANSWER✔✔-the study of nanoparticles and nanotechnology.

Nanotechnology is the use of technologies that manipulate and investigate the

properties of materials on the nanoscale.


the prefix nano refers to... - ANSWER✔✔-refers to one billionth or 10-9 in scientific

notations.

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,cation - ANSWER✔✔-metal atoms lose electrons to non metallic atoms and become

positively charged metal ions


anions - ANSWER✔✔-non metal atoms gain electrons from metal atoms and became

negatively charged non metal ions


what forces result from the attraction between positive and negative charges -

ANSWER✔✔-electrostatic


explain high melting points of ionic compounds - ANSWER✔✔-they have high melting

points because a large amount of energy is needed to overcome the electrostatic

attraction between the oppositely charges ions and allow them to move. So, the ionic

bonds between the + and - ions is strong.


explain hardness and brittleness of ionic compounds - ANSWER✔✔-a strong force is

needed to disrupt the crystal lattice, which means that it's very hard. Although a salt

crystal is hard, a strong force will shatter the crystal, meaning it's brittle. This is because

layers of ions will move relative to each other due to the force of blow. During this

movement, ions of like charge shift so they are next to each other. The repulsion

between the similarly charged ions causes the crystal to shatter


explain electrical conductivity of ionic compounds - ANSWER✔✔-in solid form, ions

are held in the crystal lattice and are not free to move, therefore don't conduct

electricity. When solids melt, the ions become free to move, enabling the cations and

anions in the molten compound to conduct electricity. When they dissolve in water,
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,ionic bonds in the lattice break and the ions are separated and move freely. When an

electric current is applied, + ions move towards the - charged electrode and - ions move

towards the + charged electrodes


properties of metals - ANSWER✔✔-Exhibit a range of melting points and relatively

high boiling points


Are good conductors of electricity


Are good conductors of heat


Generally have high densities


Are malleable - they can be shaped by beating or rolling


Are ductile - they can be drawn into a wire


Are lustrous or reflective when freshly cut or polished


Are often hard with high tensile strength


Have low ionisation energies and electronegativities




However not all metals have all of these properties


Mercury is a liquid at room temperature (low melting point)


The group 1 elements (the alkali metals) are all soft enough to be cut with a knife and

they react vigorously with water to produce hydrogen gas.

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, Both mercury and group 1 elements exhibit most of the other properties listed above.


properties of transition metals - ANSWER✔✔-Transition metals generally have unfilled

d-subshells and are often referred to as the d-block.


Their properties include


They tend to be harder


They have higher densities


They have higher melting points


Some of them have strong magnetic properties


The hardness, higher densities and higher melting points are due to the atoms of

transition metals generally being a smaller size due to their greater core charge. This

allows them to pack together more tightly with stronger bonds


what does each property say about the structure of metals


1. are hard and tend to have high boiling points


2. conduct electricity in solid and molten liquid state


3. are malleable and ductile


4. have high densities


5. good conductors of heat


6. are lustrous or reflective
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