Indicate the major type of intermolecular forces between particles in each of the following compounds.
Drag the appropriate items to their respective bins.
CHCI3
NaF
H2O
CF4
HBr
OBr2
CHCI3: Dipole-dipole forces
NaF: Ionic forces
H2O: Hydrogen bonding
CF4: Dispersion forces
HBr: Dipole-dipole forces
OBr2: Dipole-dipole forces
Explain the importance of homeostasis in the human body in a simple form
Homeostasis is important in the human body because it helps to maintain a stable internal environment. Think of it like adjusting the thermostat in your house to keep the temperature just right. In our bodies, different systems work together to keep things balanced and steady. For example, if our body temperature gets too high, we start to sweat to cool down. If our blood sugar levels go too low, our bodies release hormones to raise them back up. Homeostasis ensures that our organs and cells can work properly and stay healthy, allowing us to function at our best.
CHCI3: Dipole-dipole forces
NaF: Ionic forces
H2O: Hydrogen bonding
CF4: London dispersion forces
HBr: Dipole-dipole forces
OBr2: Dipole-dipole forces
To determine the major type of intermolecular forces between particles in each of the given compounds, we need to consider the types of bonds that hold the atoms together within each compound.
Here's a breakdown of each compound:
1. CHCI3 (Chloroform):
- Chloroform contains carbon (C), hydrogen (H), and chlorine (Cl) atoms.
- The carbon and hydrogen atoms are bonded covalently, while the chlorine atom is also covalently bonded to the carbon atom.
- The major type of intermolecular force in chloroform is dipole-dipole interactions because chlorine is more electronegative than hydrogen. This creates a partial positive charge on hydrogen and a partial negative charge on chlorine.
2. NaF (Sodium Fluoride):
- Sodium fluoride consists of sodium (Na) and fluorine (F) atoms.
- The sodium and fluorine atoms are bonded ionically, resulting in the formation of a crystal lattice structure.
- The major type of intermolecular force in NaF is called ion-dipole interactions. The positive sodium ions (Na+) and the negative fluoride ions (F-) form attractions with polar molecules.
3. H2O (Water):
- Water contains two hydrogen (H) atoms and one oxygen (O) atom.
- The hydrogen and oxygen atoms are bonded covalently, forming a bent or V-shaped molecule.
- The major type of intermolecular force in water is hydrogen bonding. The oxygen atom in water is highly electronegative, creating a partial negative charge that can form hydrogen bonds with nearby hydrogen atoms in other water molecules.
4. CF4 (Carbon Tetrafluoride):
- Carbon tetrafluoride consists of one carbon (C) atom and four fluorine (F) atoms.
- The carbon and fluorine atoms are bonded covalently, forming a tetrahedral molecule.
- The major type of intermolecular forces in CF4 are London dispersion forces. Although the CF4 molecule is nonpolar due to the symmetrical arrangement of the fluorine atoms around the carbon atom, temporary fluctuations in electron distribution can induce temporary dipoles.
5. HBr (Hydrogen Bromide):
- Hydrogen bromide consists of one hydrogen (H) atom and one bromine (Br) atom.
- The hydrogen and bromine atoms are bonded covalently.
- The major type of intermolecular force in HBr is dipole-dipole interactions, similar to CHCl3. Bromine is more electronegative than hydrogen, creating partial charges that attract each other.
6. OBr2 (Dibromine Monoxide):
- Dibromine monoxide contains two bromine (Br) atoms and one oxygen (O) atom.
- The oxygen and bromine atoms are bonded covalently.
- The major type of intermolecular force in OBr2 is also dipole-dipole interactions, similar to HBr. The oxygen atom is more electronegative than bromine, leading to partial charges and attractions between the molecules.
Therefore, the major types of intermolecular forces between particles in each compound are as follows:
CHCl3: Dipole-dipole interactions
NaF: Ion-dipole interactions
H2O: Hydrogen bonding
CF4: London dispersion forces
HBr: Dipole-dipole interactions
OBr2: Dipole-dipole interactions